Warm-up
Predict the products, determine the reaction type, and write
the balanced formula equation.
1) Silver nitrate + potassium chloride →
Type of reaction:
Balanced equation:
2) Potassium nitrate + barium chloride →
Type of reaction:
Balanced equation:
Agenda
Day
In Class
Homework
1/4
Notes: Ionic and Net Ionic
Equations
Chapter 8 WS # 1
Review Guide #1
1/6
Lab – Part I
Chapter 8 WS # 2
Review Guide # 2
Lab Report – Part I
1/10
Lab – Part II
Review Guide # 3
Lab Report – Part II
1/12
Review for Exam
Study!
Metals and Nonmetals
• Metals tend to lose electrons to form positive ions.
• Nonmetals tend to gain electrons to form negative ions.
Reactions in Aqueous Solutions
• Take place in water
• When ionic compounds dissolve in water, the resulting
solution contains the separated ions
When does a reaction occur?
1) formation of a solid (precipitation reaction)
2) formation of water (liquid)
3) transfer of electrons
4) formation of a gas
When does a solid form?
• Soluble solid – readily dissolves in water
• Ions dissociate
• Insoluble/slightly soluble – undetectable amount
dissolves
• Use solubility table on back of agenda
Net Ionic Equations
• Shows the physical states of the ions and compounds in the
reaction
• Only includes components directly involved in the reaction
• Three steps to writing net ionic equations
• Write the molecular equation
• Write the complete ionic equation
• Write the net ionic equation
Molecular Equation
• Shows complete formulas of all reactants and products,
including the physical state
• K2CrO4 (aq) + Ba(NO3)2 (aq) → BaCrO4 (s) + 2KNO3 (aq)
Complete Ionic Equation
• Represents aqueous compounds as ions
• 2K+ (aq) + CrO42- (aq) + Ba2+ (aq) + 2NO3– (aq) →
BaCrO4 (s) + 2K+ (aq) + 2NO3– (aq)
Net Ionic Equation
• Ions present on both sides of the equation and do not
participate directly in the reaction are called spectator
ions
• Not included in the net ionic equation
Ba2+ (aq) + CrO42- (aq) → BaCrO4 (s)
Acids and Bases are Aqueous
Solutions
• Strong acid – completely dissociates into H+ and the anion
• Strong base – dissociates into the cation and OH• When mixed, they always form water and a salt
Strong Acids
HI
H+(aq)
HBr
H+(aq)
HClO4
H+(aq)
HCl
H+(aq)
HClO3
H+(aq)
H2SO4
H+(aq)
HNO3
H+(aq)
Strong Bases
+
I-(aq)
+
Br-(aq)
+ ClO4
+
-(aq)
Cl-(aq)
+ ClO3
-(aq)
+ HSO4
+ NO3
-(aq)
-(aq)
NaOH
Na+(aq) + OH-(aq)
KOH
K+(aq) + OH-(aq)
LiOH
Li+(aq) + OH-(aq)
RbOH
Rb+(aq) + OH-(aq)
CsOH
Cs+(aq) + OH-(aq)
Ca(OH)2
Ca2+(aq) + 2OH-(aq)
Ba(OH)2
Ba2+(aq) + 2OH-(aq)
Sr(OH)2
Sr2+(aq) + 2OH-(aq)
Example # 1 – Hydrochloric acid and sodium hydroxide are
mixed
1 – Molecular equation
2 – Ionic equation
3 – Net ionic equation
Example # 2 – Aqueous solutions of lead (II) nitrate and
sodium sulfate are combined
1 – Molecular equation
2 – Ionic equation
3 – Net ionic equation
Example #3 – Sodium chlorate decomposes
1 – Molecular equation
2 – Ionic equation
3 – Net ionic equation
Example #4 – Methane gas (CH4) is burned in air
1 – Molecular equation
2 – Ionic equation
3 – Net ionic equation