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Net Ionic Equations

Net Ionic Equations. Writing a Complete Ionic Equation. Start with a balanced molecular equation. Break all soluble strong electrolytes (compounds with ( aq ) beside them) into their ions indicate the correct formula and charge of each ion indicate the correct number of each ion

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Net Ionic Equations

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  1. Net Ionic Equations

  2. Writing a Complete Ionic Equation • Start with a balanced molecular equation. • Break all soluble strong electrolytes (compounds with (aq) beside them) into their ions • indicate the correct formula and charge of each ion • indicate the correct number of each ion • write (aq) after each ion • Bring down all compounds with (s), (l), or (g) unchanged

  3. 2 Na3PO4 (aq) + 3 CaCl2 (aq) --> 6 NaCl (aq) + Ca3(PO4)2 (s) 6 Na+ (aq) + 2 PO43- (aq) + 3 Ca2+ (aq) + 6 Cl- (aq) --> 6 Na+ (aq) + 6 Cl- (aq) + Ca3(PO4)2 (s)

  4. Spectator Ions • Spectator ions -are present in the reaction mixture but do not participate in it. . You can recognize spectator ions by looking for ions that are present on both sides of the equation.

  5. Writing a net ionic equation Take your complete ionic equation and: • Cross out the spectator ions that are present. • Write the "leftovers" as the net ionic equation. • 6 Na+ (aq) + 2 PO43- (aq) + 3 Ca2+ (aq) + 6 Cl- (aq) --> 6 Na+ (aq) + 6 Cl- (aq) + Ca3(PO4)2 (s) • 2 PO43- (aq) + 3 Ca2+ (aq) --> Ca3(PO4)2 (s)

  6. 3 (NH4)2CO3 (aq) + 2 Al(NO3)3 (aq) --> 6 NH4NO3 (aq) + Al2(CO3)3 (s) • 2 NaOH (aq) + H2SO4 (aq) --> Na2SO4 (aq) + 2 H2O (l) • Mg (s) + 2 HCl (aq) --> MgCl2 (aq) + H2 (g) • Zn (s) + CuSO4 (aq) --> ZnSO4 (aq) + Cu (s) • Na2CO3 (aq) + 2 HNO3 (aq) --> 2 NaNO3 (aq) + H2O (l) + CO2 (g)

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