Net Ionic Equations Practice

AP Chemistry Name Net Ionic Equations Practice Period UNIT 1 – Date CHEMICAL REACTIONS Solubility Rules and Dissociation Practice For each of the ionic compounds below, determine whether or not it would be soluble (using the solubility rules). For the ones that are soluble, show how they will dissociate into ions. Some have coefficients in front— make sure to distribute these to each ion! (Remember: ionic compounds are only made of TWO ions, there shouldn’t be more than that when you break it down!) Example: 3 Na2SO4  soluble, 6 Na+ + 3 SO42- 2 AgCl  insoluble 1. 2 Ca(OH)2 ____insoluble____________ 7. 2 Al(NO3)3 __2 Al3+ + 6 NO3-_________ 2. 1 CaCO3 ____insoluble____________ 8. 3 AgI 3. 1 NaOH __1 Na+ + 1 OH-__________ 9. 1 Zn(CN)2 ____insoluble____________ ____insoluble____________ ___3 NH4+ + 3 Br-_________ 4. 3 FeF3 ____insoluble____________ 10. 3 NH4Br 5. 4 K2CO3 __8 K+ + 4 CO32-__________ 11. 2 MgCr2O7 ____insoluble____________ 6. 1 (NH4)2SO4 __2 NH4+ + 1 SO42-_______ 12. 3 Na3PO4 ___9 Na+ + 3 PO43-_________ Writing Net Ionic Equations Remember, follow these steps when writing net ionic equations. Step Example CaSO3 (s) + 2 HCl (aq)  SO2 (g) + CaCl2 (aq) + H2O (l) 1. Make sure the equation is balanced. 2. Break down all aqueous ionic compounds CaSO3 (s) + 2 H+ + 2 Cl- (aq)  SO2 (g) + Ca2+ + 2 Cl- (aq) + H2O (l) (aq) into their component ions. You can usually assume it dissociates if it says (aq). 3. Identify spectator ions—these are ions that go through no change (same state, same CaSO3 (s) + 2 H+ + 2 Cl- (aq)  SO2 (g) + Ca2+ + 2 Cl- (aq) + H2O (l) charge on both sides of the equation). Cancel out spectator ions. 4. Rewrite your equations without spectator CaSO3 (s) + 2 H+  SO2 (g) + Ca2+ + H2O (l) ions. Make sure to write charges on the leftover ions that do participate! Practice: 1. __1__ AgNO3 (aq) + __1__ NaCl (aq) → __1__ AgCl (s) + _1___ NaNO3 (aq) a. Make sure the equation is balanced. b. What type of reaction is this? ____double replacement________________________ c. Draw the particulate diagram for this reaction. Show each reactant in a separate beaker, then draw the final product together (after mixing). Include at least 3 of each ion is shown, and make sure it follows law of conservation of mass/stoichiometry. See hard copy key for diagrams d. What are the spectator ions in this reaction? ___Na+ and NO3-_________________ e. Give the net ionic equation: Ag+ + Cl-  AgCl (s) 2. __1__ Zn (s) + __2__ NiNO3 (aq)  __2__ Ni (s) + ___1_ Zn(NO3)2 (aq) a. Make sure the equation is balanced. b. What type of reaction is this? ______single replacement______________________ c. Draw the particulate diagram for this reaction. Show each reactant in a separate beaker, then draw the final product together (after mixing). Include at least 3 of each ion is shown, and make sure it follows law of conservation of mass/stoichiometry. See hard copy key for diagrams d. What are the spectator ions in this reaction? ___NO3-____________________ e. Give the net ionic equation: Zn (s) + 2 Ni+  Zn2+ + 2 Ni (s) 3. __2__ Na (s) + __2__ H2O (l)  __1__ H2 (g) + __2__ NaOH (aq) a. Make sure the equation is balanced. b. What type of reaction is this? ______single replacement______________________ c. Draw the particulate diagram for this reaction. Show each reactant in a separate beaker, then draw the final product together (after mixing). Include at least 3 of each ion is shown, and make sure it follows law of conservation of mass/stoichiometry. See hard copy key for diagrams d. What are the spectator ions in this reaction? ____none___________________ e. Give the net ionic equation: 2 Na (s) + 2 H2O (l)  H2 (g) + 2 Na+ + 2 OHAdditional Practice: On a separate sheet of paper, balance these equations & write their net ionic equations. 1. __1__ NaCl (aq) + __1__ NH4I (aq)  __1__ NaI (aq) + ___1_ NH4Cl (aq) No reaction, all the ions cancel out 2. __1__ Na2S (aq) + __2__ HCl (aq) → __2__ NaCl (aq) + __1__ H2S (g) 2 H+ + S2-  H2S (g) 3. ____ Na2CO3 (aq)+ ____ Ca(OH)2 (s) →__2__ NaOH (aq) + ____ CaCO3 (s) Ca2+ + CO32-  CaCO3 (s) 4. ____ (NH4)2SO4 (aq) + ____ Ba(NO3)2 (aq) → __2__ NH4NO3 (aq) + ____ BaSO4 (s) Ba2+ + SO42-  BaSO4 (s) 5. ____ HCl (aq) + ____ NaOH (aq) → ____ NaCl (aq) + ____ H2O (l) H+ + OH-  H2O (l) 6. ____ Na2CO3 (aq) + __2__ HCl (aq) → __2__ NaCl (aq) + ____ CO2 (g) + ____ H2O (l) CO32- + 2 H+  CO2 (g) + H2O (l)