1. Bell Ringer List the five of the most common reaction types
Describe how the law of conservation of mass is satisfied by balancing a chemical reaction.

2. The student will: SWBAT’s
Define five of the most common reaction types (synthesis/combination, decomposition, single-replacement, double displacement, and combustion).
Given a set of reactants and products, classify the reaction for five common reaction types.
Given the reactants, predict the anticipated products for the 5 basic forms of reaction types. (Example: for a basic decomposition reaction, the reactant is a binary ionic compound.)
Conduct multiple double-displacement chemical reactions in the qualitative analysis lab.
Perform the qualitative analysis lab. Using the observations from this lab, determine the identity of several unknown ionic compounds during a lab test.

3. The student will: SWBAT’s
Determine whether a single replacement reaction will occur based on a given set of reactants and the activity series. If a reaction occurs, predict the products that would be expected to form.
Use solubility rules to determine whether a given ionic compound is soluble or insoluble in water.
Given two ionic compounds as reactants, determine the substances anticipated to form and the physical state of each substance.
Describe a chemical reaction in different ways including using words and symbolic forms.
Describe how the law of conservation of mass is satisfied by balancing a chemical reaction.
Given a skeleton reaction, balance it by adding coefficients.

4. SWBAT Scale
4: Same as a 3.0 but I can make inferences & application to the SWBAT’s
3: I COMPLETELY understand all parts of the SWBAT
2: I understand MOST of the SWBAT’s with teacher help
1: I understand a little of the SWBAT’s but need teacher help
0: I do NOT understand any part of the SWBAT’s and need help!

5. Net Ionic Video’s
These show what really happens in a chemical reaction, going from the balanced equation to a net ionic equation.
1. Net Ionic Equation (Brightstorm Chemistry)
2. Bozeman Science: Molecular, Ionic, and Net Ionic Equations
3. Chemguy: Chemguy Chemistry H5F3N7
4. Mr. Causey: How to Write a Net Ionic Equation - Chemistry

6. Unit 4 “Chemical Reactions”
Adapted from: Pre-AP Chemistry
Charles Page High School
Stephen L. Cotton

7. Reactions in Aqueous Solution
OBJECTIVES:
Describe the information found in a net ionic equation.

8. Reactions in Aqueous Solution
OBJECTIVES:
Predict the formation of a precipitate in a double replacement reaction.

9. Net Ionic Equations
Many reactions occur in water- that is, in aqueous solution
When dissolved in water, many ionic compounds “dissociate”, or separate, into cations and anions

10. Net Ionic Equations
Write the molecular equation (synthesis, decomposition, etc.), then check for reactants and products that are soluble or insoluble.
We usually assume the reaction is in water
We can use a solubility table (see oxidation sheet) to tell us what compounds dissolve in water
If the compound is soluble (does dissolve in water), then the compound splits into its component ions
If the compound is insoluble (does NOT dissolve in water), then it remains as a compound

12. Net Ionic Equations
Example (needs to be a double replacement reaction) AgNO3 (aq) + NaCl(aq)  AgCl(s) + NaNO3 (aq)
1. This is the Molecular Equation
2. Next, write it as an ionic equation by splitting the compounds into their ions:
Ag1+(aq) + NO31-(aq) + Na1+(aq) + Cl1-(aq) 
AgCl (s) + Na1+(aq) + NO31-(aq)
Note that the AgCl did not ionize, because it is a “precipitate”

13. Net Ionic Equations
3. Simplify by crossing out ions not directly involved (called spectator ions)
Ag1+(aq) + Cl1- (aq)  AgCl (s)
This is called the net ionic equation

14. Net Ionic Equations Molecular Equation:
K2CrO4 + Pb(NO3)2  PbCrO KNO3
Soluble Soluble Insoluble Soluble
Net Ionic Equation:
2 K+ (aq) + CrO4-2 (aq) + Pb+2(aq) + 2 NO3-(aq) 
PbCrO4 (s) + 2 K+(aq) + 2 NO3-(aq)
*Note it remains balanced ion pairs

15. Net Ionic Equations Net Ionic Equation:
You should cancel out ions that appear on BOTH sides of the equation
2 K+(aq) + CrO4-2(aq) + Pb+2(aq) + 2 NO3-(aq) 
PbCrO4 (s) + 2 K+(aq) + 2 NO3- (aq)
CrO4-2 (aq) + Pb+2 (aq)  PbCrO4 (s)

16. Let’s do some examples together of net ionic equations, starting with these reactants:
BaCl2 + AgNO3 →
NaCl + Ba(NO3)2 →

17. Let’s do an example together of net ionic equations, starting with these reactants:
BaCl2 (aq) + 2AgNO3 (aq) → Ba (NO3) 2 (aq) + 2AgCl (s)
Ag+1 (aq) + Cl-1 (aq) → AgCl (s)
End of Unit 4

18. Let’s do some examples together of net ionic equations, starting with these reactants:
BaCl2 + AgNO3 →
NaCl + Ba(NO3)2 →