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Net Ionic Equations

This demo explores double replacement reactions in ionic compounds, focusing on why certain reactions do not occur despite the presence of reactants. We investigate reactions involving sodium chloride, silver nitrate, potassium nitrate, and others, and analyze their products based on solubility rules. The net ionic equation concept is introduced to highlight the ions that participate in the reaction. Through examples like NaCl and KBr, we evaluate whether reactions occur or result in no visible changes, referencing solubility charts for clarity.

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Net Ionic Equations

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Presentation Transcript

  1. Net Ionic Equations

  2. Do All Double Replacement Reactions Occur? (DEMO) • Sodium chloride + silver nitrate  • Sodium chloride + potassium nitrate 

  3. Why Don’t We See A Reaction? • Sometimes everything formed is soluble and dissolved in water so we don’t see it • Solubility charts give us an idea of what is soluble and what is not

  4. Are These Soluble? • Ca(OH)2 • KBr • PbCl2 • Na3(PO4)2 • MgCO3

  5. Will The Reactions Below Occur? • If the reaction occurs, write the products formed. If not write “no reaction” • NaCl + KBr  • Pb(NO3)2 + ZnCl2 • K2SO4 + CaCl2

  6. Net Ionic Reaction • Shows only the part of a replacement reaction that is actually seen • Break down all soluble substances into their ions • Cancel out ions the same on both sides of an equation – called spectator ions

  7. Write Net Ionic Reaction BaCl2 + K2SO4 Na2CO3 + Ca(OH)2 

  8. If the reactions below occur, write the net ionic equation. If not write, “no reaction” NaNO3 + KBr  BaCl2 + H2SO4  CaBr2 + Na2CO3  Ag(NO3) + NaCl 

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