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Net Ionic Equations. Net-ionic Equations  Net ionic equations are useful in that they show only those chemical species directly participating in a chemical.

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Presentation on theme: "Net Ionic Equations. Net-ionic Equations  Net ionic equations are useful in that they show only those chemical species directly participating in a chemical."— Presentation transcript:

1 Net Ionic Equations

2 Net-ionic Equations  Net ionic equations are useful in that they show only those chemical species directly participating in a chemical reaction  The keys to being able to write net ionic equations are the ability to recognize monatomic and polyatomic ions, the solubility rules, and the rules for electrolyte behavior.

3 Net ionic equations  Complete ionic equations  An ionic equation that shows all of the particles in a solution as they realistically exist  2 Na + (aq) + 2OH- (aq) + Cu +2 (aq) + 2Cl - (aq)  2 Na + (aq) + 2 Cl - (aq) + Cu(OH) 2 (s)  Note that the sodium ions and the chloride ions are both reactants and products, therefore they do not participate in the reaction  Ions that do not participate in the reaction are called spectator ions

4 Net-ionic Equations  Ionic equations that include only the particles that participate in the reaction are called net ionic equations  Net ionic equations are written form complete ionic equations by crossing out all spectator ions  Example:  2 Na + (aq) + 2OH- (aq) + Cu +2 (aq) + 2Cl - (aq)  2 Na + (aq) + 2 Cl - (aq) + Cu(OH) 2 (s)

5 Net-ionic Equations  A net ionic equation is what remains after the sodium and chloride ions are crossed out of this complete ionic equation  2OH - (aq) + Cu +2 (aq)  Cu(OH) 2  Only the hydroxide and copper ions are left in the net ionic equation shown above

6 Example:  Write the chemical, complete ionic, and net ionic equations for the rxn between aqueous solutions of barium nitrate and sodium carbonate that forms the precipitate barium carbonate.  Complete Ionic Equation:  Ba(NO 3 ) 2 (aq) + Na 2 CO 3 (aq)  BaCO 3 (s) + NaNO 3 (aq)  Balance the equation above:  Ba(NO 3 ) 2 (aq) + Na 2 CO 3 (aq) + BaCO 3 (s) + 2 NaNO 3 (aq)

7 Example continued:  Show the ionic states of the reactants and products  Ba +2 (aq) + 2NO 3 - (aq) + 2Na + + CO 3 -2 (aq)  BaCO 3 (s) + 2 Na + (aq) + 2NO 3 - (aq)  Cross out the spectator ions from the complete ionic equation:  Ba +2 (aq) + 2NO 3 - (aq) + 2Na + + CO 3 -2 (aq)  BaCO 3 (s) + 2 Na + (aq) + 2NO 3 - (aq)

8 Example continued:  The net ionic equation is:  Ba +2 (aq) + CO 3 -2 (aq)  BaCO 3 (s)

9 Practice  Work on problems 33-36 on pg. 294 of your chemistry book


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