Net Ionic Equations Writing a Complete Ionic Equation

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 – write (aq) after each ion • Bring down all compounds with (s), (l), or (g) unchanged

2 Na 3 PO 4 (aq) + 3 Ca. Cl 2 (aq) --> 6 Na. Cl (aq) + Ca 3(PO 4)2 (s) 6 Na+ (aq) + 2 PO 43 - (aq) + 3 Ca 2+ (aq) + 6 Cl- (aq) --> 6 Na+ (aq) + 6 Cl- (aq) + Ca 3(PO 4)2 (s)

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.

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 PO 43 - (aq) + 3 Ca 2+ (aq) + 6 Cl(aq) --> 6 Na+ (aq) + 6 Cl- (aq) + Ca 3(PO 4)2 (s) • 2 PO 43 - (aq) + 3 Ca 2+ (aq) --> Ca 3(PO 4)2 (s)

• 3 (NH 4)2 CO 3 (aq) + 2 Al(NO 3)3 (aq) --> 6 NH 4 NO 3 (aq) + Al 2(CO 3)3 (s) • 2 Na. OH (aq) + H 2 SO 4 (aq) --> Na 2 SO 4 (aq) + 2 H 2 O (l) • Mg (s) + 2 HCl (aq) --> Mg. Cl 2 (aq) + H 2 (g) • Zn (s) + Cu. SO 4 (aq) --> Zn. SO 4 (aq) + Cu (s) • Na 2 CO 3 (aq) + 2 HNO 3 (aq) --> 2 Na. NO 3 (aq) + H 2 O (l) + CO 2 (g)