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Net Ionic Equation Worksheet: Honors Chemistry, Study notes of Chemistry

Chemistry

Directions: Write balanced molecular, ionic, and net ionic equations for each of the following reactions. Assume all reactions occur in aqueous solution.

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Honors Chemistry Name__________________________________ Period_____
Net Ionic Equation Worksheet
READ THIS: When two solutions of ionic compounds are mixed, a solid may form. This type of reaction is called a precipitation reaction, and the solid produced
in the reaction is known as the precipitate. You can predict whether a precipitate will form using a list of solubility rules such as those found in the table below.
When a combination of ions is described as insoluble, a precipitate forms. There are three types of equations that are commonly written to describe a
precipitation reaction.
The molecular equation shows each of the substances in the reaction as compounds with physical states written next to the chemical formulas. The
complete ionic equation shows each of the aqueous compounds as separate ions. Insoluble substances are not separated and these have the symbol (s) written
next to them. Water is also not separated and it has a (l) written next to it. Notice that there are ions that are present on both sides of the reaction arrow –>
that is, they do not react. These ions are known as spectator ions and they are eliminated from complete ionic equation by crossing them out. The remaining
equation is known as the net ionic equation. For example: The reaction of potassium chloride and lead II nitrate
Molecular Equation: 2KCl (aq) + Pb(NO3)2 (aq) -> 2KNO3 (aq) + PbCl2 (s)
Complete Ionic Equation: 2K+ (aq) + 2Cl- (aq) + Pb2+ (aq) + 2NO3– (aq) -> 2K+ (aq) + 2NO3– (aq) + PbCl2 (s)
Net Ionic Equation: 2Cl- (aq) + Pb2+ (aq) -> PbCl2 (s)
Directions: Write balanced molecular, ionic, and net ionic equations for each of the following reactions. Assume all reactions occur in aqueous solution. Include
states of matter in your balanced equation.
1. Sodium chloride and lead II nitrate
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
2. Sodium carbonate and Iron II chloride
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
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Honors Chemistry Name__________________________________ Period_____ Net Ionic Equation Worksheet READ THIS: When two solutions of ionic compounds are mixed, a solid may form. This type of reaction is called a precipitation reaction , and the solid produced in the reaction is known as the precipitate. You can predict whether a precipitate will form using a list of solubility rules such as those found in the table below. When a combination of ions is described as insoluble, a precipitate forms. There are three types of equations that are commonly written to describe a precipitation reaction. The molecular equation shows each of the substances in the reaction as compounds with physical states written next to the chemical formulas. The complete ionic equation shows each of the aqueous compounds as separate ions. Insoluble substances are not separated and these have the symbol ( s ) written next to them. Water is also not separated and it has a ( l ) written next to it. Notice that there are ions that are present on both sides of the reaction arrow – > that is, they do not react. These ions are known as spectator ions and they are eliminated from complete ionic equation by crossing them out. The remaining equation is known as the net ionic equation. For example : The reaction of potassium chloride and lead II nitrate Molecular Equation: 2KCl ( aq ) + Pb(NO 3 ) 2 ( aq ) - > 2KNO 3 ( aq ) + PbCl 2 ( s ) Complete Ionic Equation: 2K+^ ( aq ) + 2Cl-^ ( aq ) + Pb2+^ ( aq ) + 2NO^3 –^ ( aq ) - > 2K+^ ( aq ) + 2NO 3 –^ ( aq ) + PbCl 2 ( s ) Net Ionic Equation: 2Cl-^ ( aq ) + Pb2+^ ( aq ) - > PbCl 2 ( s ) Directions: Write balanced molecular, ionic, and net ionic equations for each of the following reactions. Assume all reactions occur in aqueous solution. Include states of matter in your balanced equation.

  1. Sodium chloride and lead II nitrate Molecular Equation: Complete Ionic Equation: Net Ionic Equation:
  2. Sodium carbonate and Iron II chloride Molecular Equation: Complete Ionic Equation:
  1. Magnesium hydroxide and hydrochloric acid Molecular Equation: Complete Ionic Equation: Net Ionic Equation:
  2. Potassium chromate and calcium chloride Molecular Equation: Complete Ionic Equation: Net Ionic Equation:
  3. Ammonium phosphate and zinc nitrate Molecular Equation: Complete Ionic Equation: Net Ionic Equation:
  4. Lithium hydroxide and barium chloride Molecular Equation: Complete Ionic Equation:
  1. Silver nitrate and magnesium iodide Molecular Equation: Complete Ionic Equation: Net Ionic Equation:
  2. Ammonium chromate and aluminum perchlorate Molecular Equation: Complete Ionic Equation: Net Ionic Equation:
  3. Nickel nitrate and sodium hydroxide Molecular Equation: Complete Ionic Equation:
  1. Hydrobromic acid (HBr) and lead II perchlorate Molecular Equation: Complete Ionic Equation: Net Ionic Equation:
  2. Potassium fluoride and magnesium nitrate Molecular Equation: Complete Ionic Equation: Net Ionic Equation:
  3. Sodium phosphate and nickel II perchlorate Molecular Equation: Complete Ionic Equation: Net Ionic Equation:
  4. Copper II chloride and silver acetate Molecular Equation: Complete Ionic Equation:
  1. Molecular Equation: 2 FeCl 3 (aq) + 3 Mg(s)  3 MgCl 2 (aq) + 2 Fe(s) Ionic Equation: 2 Fe3+(aq) + 6 Cl-(aq) + 3 Mg(s)  3 Mg2+(aq) + 6 Cl-(aq) + 2 Fe(s) NIE: 2 Fe3+(aq) + 3 Mg(s)  3 Mg2+(aq) + 2 Fe(s)
  2. Molecular Equation: BaBr 2 (aq) + Na 2 SO 4 (aq)  BaSO 4 (s) + 2 NaBr(aq) Ionic Equation: Ba2+(aq) + 2 Br-(aq) + 2 Na+(aq) + SO 42 - (aq)  BaSO 4 (s) + 2 Na+(aq) + 2 Br-(aq) NIE: Ba2+(aq) + SO 42 - (aq)  BaSO 4 (s)
  3. Molecular Equation: 2 AgNO 3 (aq) + MgI 2 (aq)  2 AgI(s) + Mg(NO 3 ) 2 (aq) Ionic Equation: 2 Ag+(aq) + 2 NO 3 - (aq) + Mg2+(aq) + 2 I-(aq)  2 AgI(s) + Mg2+(aq) + 2 NO 3 - (aq) NIE: 2 Ag+(aq) + 2 I-(aq)  2 AgI(s) (your final answer would be: Ag+(aq) + I-(aq)AgI(s) )
  4. Molecular Equation: 3 (NH 4 ) 2 CrO 4 (aq) + 2 Al(ClO 4 ) 3 (aq)  Al 2 (CrO 4 ) 3 (s) + 6 NH 4 ClO 4 (aq) Ionic Equation: 6 NH 4 +(aq) + 3 CrO 42 - (aq) + 2 Al3+(aq) + 6 ClO 4 - (aq)  6 NH 4 +(aq) + 6 ClO 4 - (aq) + Al 2 (CrO 4 ) 3 (s) NIE: 3 C 2 O 42 - (aq) + 2 Al3+(aq)  Al 2 (CrO 4 ) 3 (s)
  5. Molecular Equation: Ni(NO 3 ) 2 (aq) + 2 NaOH(aq)  Ni(OH) 2 (s) + 2 NaNO 3 (aq) Ionic Equation : Ni2+(aq) + 2 NO 3 - (aq) + 2 Na+(aq) + 2 OH-(aq)  Ni(OH) 2 (s) + 2 Na+(aq) + NO 3 - (aq) NIE: Ni2+(aq) + 2 OH-(aq)  Ni(OH) 2 (s)
  6. Molecular Equation: 2 HBr(aq) + Pb(ClO 4 ) 2 (aq)  2 HClO 4 (aq) + PbBr 2 (s) Ionic Equation: 2 H+(aq) + 2 Br-(aq) + Pb2+(aq) + 2ClO 4 - (aq)  2H+(aq) + 2 ClO 4 - (aq) + PbBr 2 (s) NIE: 2 Br-(aq) + Pb2+(aq)  PbBr 2 (s)
  7. Molecular Equation: 2 KF(aq) + Mg(NO 3 ) 2 (aq)  2 KNO 3 (aq) + MgF 2 (s) Ionic Equation: 2 K+(aq) + 2 F-(aq) + Mg2+(aq) + 2NO 3 - (aq)  2 K+(aq) + 2 NO 3 - (aq) + MgF 2 (s) NIE: 2 F-(aq) + Mg2+(aq)  MgF 2 (s)
  8. Molecular Equation: 2 Na 3 PO 4 (aq) + 3 Ni(ClO 4 ) 2 (aq)  6 NaClO 4 (aq) + Ni 3 (PO 4 ) 2 (s) Ionic Equation: 6 Na+(aq) + 2 PO 43 - (aq) + 3 Ni2+(aq) + 6 ClO 4 - (aq)  6 Na+(aq) + 6 ClO 4 - (aq) + Ni 3 (PO 4 ) 2 (s) NIE : 2 PO 43 - (aq) + 3 Ni2+(aq)  Ni 3 (PO 4 ) 2 (s)
  9. Molecular Equation: CuCl 2 (aq) + 2 AgC 2 H 3 O 2 (aq)  Cu(C 2 H 3 O 2 ) 2 (aq) + 2 AgCl(s) Ionic Equation: Cu2+(aq) + 2 Cl-(aq) + 2 Ag+(aq) + 2 C 2 H 3 O 2 - (aq)  Cu2+(aq) + 2 C 2 H 3 O 2 - (aq) + 2 AgCl(s) NIE: Cl-(aq) + Ag+(aq)  AgCl(s)