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Net Ionic Equations

Learn about various chemical reactions including .Net Ionic Equations, Double Replacement, Redox, Single Replacement, Composition, and Decomposition. Understand the identification of reactions, acid/base reactions, and complex ions. Practice balancing equations and identifying reaction types.

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Net Ionic Equations

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  1. Net Ionic Equations Double Replacement Redox / Single Replacement Composition/Decomposition Complex Ions Combustion

  2. Identification of Double Replacement Reaction • Acid / Base NH3 + HF  NH4+ + F – • Precipitation Ba2+ + SO42- BaSO4 • Both 2 H+ + SO42- + Ca(OH)2 CaSO4 + 2 HOH

  3. Redox and Single Replacement Redox • Use of key terms MnO4- H2O2 Cr2O72- HNO3 • Elements with multiple oxidation states Sn2+ Sn4+ Cr2+ Cr3+ Cr6+ I- IO- IO2- O(-1 or -2) • Acidic and Basic conditions 4 MnO4- + 12 H+ + 20 H2O2 4 Mn2+ + 15 O2 + 26 H2O

  4. Redox / Single Replacement Single Replacement • Like will replace like 2 Na + 2 H2O  2 Na+ + 2 OH- + H2 Cl2 + 2 KI  2 K+ + 2 Cl- + I2

  5. Combustion • Reaction of a hydrocarbon/alcohol or other organic molecule with oxygen gas to produce carbon dioxide and water C3H8 + 5 O2→ 3 CO2 + 4 H2O CH3CH2OH + 3 O2 → 2 CO2 + 3 H2O

  6. Decomposition/Composition • Decomposition has only one reactant and it breaks up into elements and /or compounds MgCO3 MgO + CO2 Ba(OH)2  BaO + H2O 2 Al2O3  4 Al + 3 O2

  7. Decomposition / Composition • Composition has two reactants that combine into one product S8 + 8 O2 8 SO2 • nonmetal oxides plus water makes acids SO3 + H2O  2 H++SO42- • metal oxides plus water makes bases CaO + H2O  Ca(OH)2

  8. Complex Ions • Particles that generally combine with excess ligand (often water, hydroxide or ammonia) to form complex ions with a charge Cu2+ + 4 NH3 [Cu(NH3)4]2+ Al3+ + 4 OH-  [Al(OH)4]- AgCl + 2 NH3 [Ag(NH3)2]+ + Cl- Fe3++ SCN- [Fe(SCN)]2+ having the correct ligand number is not required but being consistent with number and charge is important

  9. In Review • Identify type of reaction from list of 5 types • Equations need to be balanced • Check for appropriate charges • Remember not to include spectator ions • Remember practice questions about each of the 3 balanced net ionic equations

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