1. Chemical Equations Main Concept:
A chemical change may be represented by a molecular, ionic, or net ionic equation.

2. Chemical Equations Chemical Equations Types of Chemical Equations
Balanced Molecular
Ionic
Net Ionic
Types of Chemical Reactions

3. - Chemical equations represent chemical changes
- they must contain equal numbers of atoms of every element on each side to be “balanced”

4. - Depending on context, there are different forms of the balanced chemical equations
- Be aware of the different forms: balanced molecular, ionic, or net ionic reaction equation
- Know circumstances under which any of them might be the most useful form

5. Pb2+ (aq) + 2 NO32- (aq) + 2 K+ (aq) + 2 I- (aq) 
- Balanced Molecular Equation:
- most equations you’ve used
Pb(NO3)2 (aq) + 2 KI (aq)  PbI2 (s) + 2 KNO3 (aq)
- Ionic Equation (Complete Ionic Equation):
- ions dissolved in solutions
Pb2+ (aq) + 2 NO32- (aq) + 2 K+ (aq) + 2 I- (aq) 
PbI2 (s) + 2 K+ (aq) + 2 NO3- (aq)

6. Pb2+ (aq) + 2 NO32- (aq) + 2 K+ (aq) + 2 I- (aq) 
PbI2 (s) + 2 K+ (aq) + 2 NO3- (aq)
- Net Ionic Reaction Equation
- like ionic equation, but focusing only on the
important ions
- often useful for redox reactions
Pb2+ (aq) + 2 I- (aq)  PbI2 (s)

7. Equation Practice

8. - A balanced equation for a reaction can represent chemistry at any level
*** You should be able to translate into a symbolic depiction at the particulate level

9. Synthesis and Decomposition Reactions
Main Concept:
Synthesis reactions are those in which atoms and/or molecules combine to form a new compound.  

10. Synthesis Reactions
C + O2  CO2
CaO + H2O  Ca(OH)2
2CO + O2  2CO2

11. Decomposition Reactions
Decomposition is the reverse of synthesis, a process whereby molecules are decomposed, often by the use of heat.

12. Decomposition Reactions
H2CO  H2O + CO2
H2SO3  H2O + SO2
NH4OH  H2O + NH3

13. Decomposition Reactions
2H2O  2H2 + O2
C12H22O11  12C + 11H2O
2H2O2  2H2O + O2

14. Single Replacement Reactions
Cu + 2AgNO3  2Ag + Cu(NO3)2
Fe + Cu(NO3)2  Fe(NO3)2 + Cu
Ca + 2H2O  Ca(OH)2 + H2

15. Double Replacement Reactions
2KOH + H2SO4  K2SO4 + 2H2O
FeS + 2HCl FeCl2 + H2S
AgNO3 + NaCl  AgCl + NaNO3

16. Stoichiometry Main Concept:
Quantitative information can be derived from stoichiometric calculations utilizing mole ratios from the balanced chemical equations.  Stoichiometry has real-world applications.

17. - Coefficients of balanced chemical equations contain information regarding proportionality of amounts of substances involved in reaction
- Values can be used in chemical calculations that apply the mole concept
- The most important place for this is the laboratory.

18. With stoichiometry, we can…
- Calculate amount of product expected be produced in laboratory experiments
- Identify limiting and excess reactant; calculate percent and theoretical yield for a given laboratory experiment.

19. With stoichiometry, we can…
- Investigate gases, particularly with respect to the experimental determination of molar mass of a gas.
- Better understand solution chemistry, including titrations.