Post on 17-Jan-2018
description
Ionic Equations• Most ionic compound dissociate
(or break apart) when dissolved in water to form its component ions
• For example: NaCl (aq) really looks like Na+(aq) and Cl- (aq)
Soluble Vs. Precipitate• Soluble means that the compound breaks
down into its ions in water• Ex) NaCl is soluble so it forms Na+ and Cl-• Insoluble means that the compound
doesn’t break down in water
Precipitate Reactions• In double replacement reactions,
often one of the product will be insoluble
• The insoluble product is referred to as a precipitate.
AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
What happens when you put
AgNO3 and NaCl in water?
AgNO3NaCl
AgNO3NaCl
AgNO3 NaCl
AgNO3 NaCl
AgNO3 NaCl
AgNO3 NaCl
AgNO3 NaCl
Ag NO3 Na Cl
Ag+ NO3- Na+ Cl-
Ag+ NO3- Na+ Cl-
Ag+ NO3- Na+ Cl-
Ag+ NO3- Na+
Cl-
Ag+NO3
-Na+
Cl-
Ag+
NO3-
Na+
Cl-
Ag+
NO3-
Na+
Cl-
Ag+
NO3-
Na+
Cl-
Ag+
NO3-
Na+
Cl-
Ag+
NO3- Na+
Cl-
Ag+
NO3-
Na+
Cl-
Ag+
NO3-
Na+
Cl-
Ag+
NO3-
Na+
Cl-
AgCl
NO3- Na+
AgCl
NO3-
Na+
AgCl
NO3-
Na+
AgCl
NO3-
Na+
AgCl(s)precipitate
AgCl
NO3-
Na+
AgCl(s)precipitate
AgCl
NO3-
Na+
AgCl
NO3- Na+
AgCl
NO3- Na+
AgCl
NO3- Na+
AgCl
NO3- Na+
AgCl
NO3-
Na+
AgCl
NO3-
Na+
AgCl
NO3-
Na+
AgCl
NO3-
Na+
AgNO3
NaCl
AgNO3
NaCl
AgNO3
NaClAgNO3
NaClAgNO3
NaCl AgNO3NaCl AgNO3 NaCl
AgNO3
NaCl
AgNO3
NaCl
AgNO3
NaClAgNO3
NaClAgNO3
NaCl AgNO3NaCl AgNO3 NaCl
AgNO3
NaCl
AgNO3
NaCl
AgNO3
NaClAgNO3
NaClAgNO3
NaCl AgNO3NaCl AgNO3 NaCl
Ag+ NO3- Na+ Cl-
AgNO3
NaCl
AgNO3
NaCl
AgNO3
NaClAgNO3
NaClAgNO3
NaCl AgNO3NaCl AgNO3 NaCl
Ag+ NO3- Na+ Cl-
NaClNaClAgNO3NaCl AgNO3NaCl AgNO3
Ag+ NO3-
Na+
Cl-
Ag+
NO3-
Na+Cl-
AgCl
Ag+ NO3- Na+ Cl-
Ag+NO3-
Na+
Cl- Ag+
NO3-
Na+
Cl-
Ag+NO3
-Na+
Cl-
Ag+
NO3-
Na+
Cl-Ag+
NO3-
Na+
Cl-Cl-Ag+
AgClAgCl AgCl
Ag+Cl-Cl- Ag+
NO3-
Na+
Cl-
NO3-
Na+Ag+
NO3-
Na+
Ag+NO3
-Na+
Cl-
Na+NO3
-
Na+
Cl- Ag+
NO3-
Na+
NO3-
Na+
Cl-
NO3-
Na+
AgClAgClAgClAgCl
Ag+
Cl-Ag+
Cl-
Ag+Cl- Ag+
NO3-
Na+
NO3-
Na+Ag+
NO3-
Na+
Ag+NO3
-Na+
Cl-
Na+NO3
-
Na+
NO3-
Na+
NO3- Na+
Cl-
NO3-
Na+
Ag+Cl-
Ag+
Cl-
NO3-
Na+
NO3-
Na+Ag+
NO3-
Na+
Ag+NO3
-Na+
Cl-
Na+NO3
-
Na+
NO3-
Na+
NO3- Na+
Cl-
NO3-
Na+
NO3-
Na+
NO3-
Na+Ag+
NO3-
Na+
Ag+NO3
-Na+
Cl-
Na+NO3
-
Na+
NO3-
Na+
NO3- Na+
Cl-
NO3-
Na+
NO3-
Na+
NO3-Na+
NO3-Na+NO3
-Na+Na+ NO3
-
Na+
NO3-
Na+
NO3-
Na+
NO3-
Na+
NO3-
Na+
NO3-Na+
NO3-
Na+NO3-Na+Na+ NO3
-
Na+
NO3- Na+
NO3-
Na+
NO3-
Na+
AgCl(s)
NO3-
Na+
NO3-Na+
NO3-Na+NO3
-Na+Na+ NO3
-
Na+
NO3-
Na+
NO3-
Na+
NO3-
Na+
AgCl(s)
NO3-
Na+
NO3-Na+
NO3-
Na+NO3-Na+Na+ NO3
-
Na+
NO3- Na+
NO3-
Na+
NO3-
Na+
AgCl(s)
Ionic Equations Continued• To write a Complete Ionic Equation:• Write the aqueous substances as ions
(leave any substances in gas, liquids, & solids alone)
• Example:• AgNO3 (aq) + NaCl (aq) AgCl (s) +
NaNO3 (aq)
Spectator Ions• Spectator Ions-Ions that are not
directly involved in a reaction• Spectator ions show up on both
sides of the equation• Spectator Ions cancel out
NET Ionic Equations• Net Ionic Equation-Indicate the
particles that actually take part in a reaction
• The Net Ionic Equation does NOT include spectator ions
• Net Ionic Equations must be balanced according to atoms and charge
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
ionic equation
AgNO3 NaCl
Ag NO3 Na Cl
Ag+ NO3- Na+ Cl-
Ag+ NO3- Na+ Cl-
Ag+ NO3- Na+ Cl-
Ag+ NO3- Na+
Cl-
Ag+NO3
-Na+
Cl-
Ag+
NO3-
Na+
Cl-
Ag+
NO3-
Na+
Cl-
Ag+
NO3-
Na+
Cl-
Ag+
NO3-
Na+
Cl-
Ag+
NO3- Na+
Cl-
Ag+
NO3-
Na+
Cl-
Ag+
NO3-
Na+
Cl-
Ag+ Cl-
NO3- Na+
Reaction
NO3- Na+
AgClReaction
NO3- Na+
AgCl
AgCl
NO3- Na+
No Reaction
AgCl
NO3- Na+
No Reaction
AgCl
NO3-
Na+
No Reaction
AgCl
NO3- Na+
AgCl
NO3- Na+
AgCl
NO3- Na+
AgCl
NO3- Na+
AgCl
NO3- Na+
AgCl
NO3- Na+
These ions do not participatein the reaction. They are called
SPECTATOR IONS
Ag+Cl-
Ag+ Cl-
Ag+ Cl-
Ag+Cl-
Ag+ Cl-
Ag+Cl-
Ag+ Cl-
Ag+ Cl-
AgCl
AgCl
AgCl
AgCl
AgCl
AgCl
AgCl
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
The net ionic equation is constructed from the ionic equation:
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
No3- and Na+ are not participating in the reaction
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
net ionic equation
Ag+ (aq) + Cl- (aq)
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
net ionic equation
Ag+ (aq) + Cl- (aq)
Ag+ and Cl- are reacting to form
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
net ionic equation
Ag+ (aq) + Cl- (aq)
Ag+ and Cl- are reacting to form
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
net ionic equation
Ag+ (aq) + Cl- (aq) AgCl (s)
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
net ionic equation
Ag+ (aq) + Cl- (aq) AgCl (s)