Net Ionic Equations
How do we write chemical
equations?
• Potassium chloride reacts with
Sodium fluoride to produce
potassium fluoride and sodium
chloride.
3 Forms of Chemical
Equations
1) Molecular
o Form you are most familiar with
o Reactants and products written as
neutral compounds
o Ex. KCl + NaF  NaCl + KF
Chemical Equations (cont.
)
2) Full Ionic
o All chemical compounds are written as
ions if they can be (ex. Strong electrolytes,
strong acids, strong bases, etc.)
o Soluble compounds—dissociate into ions
o Insoluble compounds—solid precipitate
o USE SOLUBILITY RULES!!!
o Ex. Ba+2 + 2Cl- + 2Na+
+
(s) + 2Na + 2Cl
+ SO4-2  BaSO4
How do we write a FULL
IONIC equation?
• Insoluble compounds are written as SOLIDS
• Pure liquids and gases are written as is, not
broken up into ions, electrically neutral.
• Which compounds are broken up into ions????
o Soluble ionic compounds
o Strong acids (HCl, HBr, HI, HNO3 , HClO4 , H2SO4)
o Strong Bases ( Group IA bases and Ca(OH)2, Sr(OH)2 , Ba(OH)2
Ex 1. Na2CrO4 + Pb(NO3)2
2NaNO3
• Write the full ionic equation.
PbCrO4 +
Ex. 2: 2CH3CO2H + Sr(OH)2 
Sr(CH3CO2)2 + 2H2O
• Write the full ionic equation
Forms of Chemical
Equations (cont.)
3) Net Ionic Equations
o Next step after full ionic equation.
o Elimination of Spectator Ions (ions
found on both sides of the equation,
not changed with reaction)
o Includes chemical compounds and
ions DIRECTLY involved in chemical
reaction.
From Example 1:
• 2Na+ + CrO4-2 + Pb+2 +
+ 2Na+ + 2NO3-
• Write the net ionic equation.
2NO3-
 PbCrO4 (s)
From Example 2:
• 2CH3CO2H + Sr+2
2CH3CO2- + 2H2O
+
• Write net ionic equation.
2OH-  Sr+2 +
Putting it ALL together ! ! !
Example 3:
Na2CO3 + Ca(NO3)2

Write net ionic equation
2NaNO3 +
CaCO3 (s)
Example 4:
• Magnesium metal reacts with HCL to produce a
solution of magnesium chloride and hydrogen gas.
• Write the molecular equation and net ionic
equation.
Homework
• Net Ionic Equation worksheet.