1. As you come in, Materials: Plan:
Paper, periodic table, and pencil for the test
Plan:
Complete the Unit Four Bonding test
Read the Chemical Literacy #4 article and respond to the questions. (due tomorrow)
Go to Edmodo, and begin the assignments.
DUE TOMORROW – Balancing Equations note-taking guide
DUE THURSDAY – Types of Equations note-taking guide
DUE FRIDAY – Predicting Products note-taking guide
Begin writing chemical equations on the “Writing Equations from Word Equations” handout.

2. As you come in, Materials: Chemical Literacy Answers
Balancing Equations Note-taking Guide
Practice Packet (pick up at front)
Periodic table and paper for notes
Plan:
Learn to write and balance chemical equations
Complete the “Writing Equations from Word Equations” handout
Continue practicing handouts listed on “1c” of SLA list
Tonight:
Go to Edmodo.
DUE TOMORROW – Types of Equations note-taking guide
DUE FRIDAY – Predicting Products note-taking guide

3. Chemical Reactions
Process by which the atoms of one or more substances are rearranged to form different substances
Law of Conservation of Matter – Matter is not created or destroyed during a chemical reaction.

4. Writing Chemical Equations
Video Example 1:
Combustion of H2 gas
Description: Hydrogen gas burns in oxygen gas to produce water vapor.
Unbalanced equation:
Read a description of the reaction
Note what is reacted with what
Note what is yielded or produced
Write formulas for each compound
Use + to represent “and”
Use  to represent “produces” or “yields”
Include states of matter where available
(s) solid
(l) liquid
(g) gas
(aq) dissolved in water
Video Example 2:
Combustion of methane gas
Description: Methane gas burns in oxygen gas to produce carbon dioxide and water vapor.
Unbalanced equation:

5. Balancing Chemical Equations
Video Example 1:
Combustion of H2 gas
Unbalanced equation:
H2 + O2  H2O
Balanced equation:
Write the skeleton equation.
BE SURE THE FORMULAS ARE WRITTEN CORRECTLY.
Inventory reactants
Inventory products
Insert coefficients to make atoms of each element equal on both sides of the equation
Reduce the coefficients if possible
Video Example 2:
Combustion of methane gas
Unbalanced equation:
CH4 + O2  CO2 + H2O
Balanced equation:

6. Guided Example
Sodium carbonate reacts with chromium (III) chloride to produce sodium chloride and chromium (III) carbonate.
Unbalanced Equation:
Na2CO3 + CrCl3  NaCl + Cr2(CO3)3
Balanced Equation:
3Na2CO3 + 2CrCl3  6NaCl + Cr2(CO3)3

7. Writing Equations from Word Equations handout
Work with a partner to write and balance equations.
Take 10 minutes to write and balance as many as possible.
Use a colored pencil or pen to correct your mistakes.

8. Writing & Balancing Equations
Zn + Pb(NO3)2 --> Zn(NO3)2 + Pb
2 AlBr3 + 3 Cl2 --> 2 AlCl3 + 3 Br2
2 Na3PO4 + 3 CaCl2 --> Ca3(PO4) NaCl
2 K + Cl2 --> 2 KCl
2 Al + 6 HCl --> 2 AlCl3 + 3 H2
3 Ca(OH)2 + 2 H3PO4 --> Ca3(PO4)2 + 6 H2O
Cu + 2 H2SO4 --> CuSO4 + 2 H2O + SO2
2 H2 + 2 NO --> 2 H2O + N2

9. As you come in, a Materials: Types of Reactions Note-taking Guide
Periodic table and paper for notes
Plan:
Balancing more advanced equations
Learn about types of equations
Practice identifying types of equations and writing equations
Practice balancing for tomorrow’s quiz
Tonight:
Go to Edmodo.
DUE TOMORROW– Predicting Products note-taking guide
Practice balancing equations for tomorrow’s quiz!

10. Difficult Equations to Balance
Copper and sulfuric acid react to form copper (II) sulfate and water and sulfur dioxide.
Cu + 2 H2SO4 --> CuSO4 + 2 H2O + SO2

11. 5 Types of Chemical Reactions
Synthesis A + B  AB
Combustion CxHy + O2  CO2 + H2O
Decomposition AB  A + B
Double-Replacement AX + BY  AY + BX
Single-Replacement A + BX  B + AX
Five Types of Reactions Clip

12. Identify the Type of Reaction
Zn + Pb(NO3)2 --> Zn(NO3)2 + Pb
2KClO3  2KCl +3 O2
2 AlBr3 + 3 Cl2 --> 2 AlCl3 + 3 Br2
2 Na3PO4 + 3 CaCl2 --> Ca3(PO4) NaCl
2 K + Cl2 --> 2 KCl
2 Al + 6 HCl --> 2 AlCl3 + 3 H2
CH4 + 2O2  CO2 + 2H2O
3 Ca(OH)2 + 2 H3PO4 --> Ca3(PO4)2 + 6 H2O

13. Single Replacement Reactions SPECIAL! MORE TO COME!
A + BX --> AX + B
A metal will not always replace another metal. The reactivity of the metal is important to consider.
Reaction: More active metal replaces a less active metal.
No Reaction: A less active metal will not replace a more active metal.
Use the metal activity series to determine if single replacement reactions occur.
Find the element who is alone in the reactants on the series.
Identify the element that is most similar to it in the reactant compound.
The LONE element must be HIGHER than the compound element.

14. Work with a partner to Identify type of reaction and write equations.
“Long worksheet” #26-50
Work with a partner to Identify type of reaction and write equations.
Take 10 minutes to identify types and write as many as possible.
Use a colored pencil or pen to correct your mistakes.

15. “Balancing Chemical Equations” handout
Work with a partner to Balance the equations. Your quiz will be similar to this tomorrow.
Take 10 minutes to balance as many as possible.
Use a colored pencil or pen to correct your mistakes.

16. As you come in, Materials: Paper for quiz
Predicting Products note-taking guide
Plan:
Balancing Equations Quiz (TIME LIMIT: 30 minutes)
Practice writing, balancing, and identifying types of reactions
Learn to predict the products of double and single replacement reactions
Discovery Lab – Indicators of a Chemical Reaction
Tonight:
Go to Edmodo.
DUE MONDAY– Net Ionic Equations note-taking guide
Practice identifying the types reactions for Monday’s quiz!

17. AFTER YOUR QUIZ
Write, balance, and identify the type of reaction for the following on your “LONG worksheet”
#26-#50
(as many as you can)

18. Predicting Products & States of Matter
Expectations:
To predict the products of DOUBLE REPLACEMENT and SINGLE REPLACEMENT reactions
To use the Solubility Rules to predict the states of matter of your products

19. Let’s add states of matter.
Predicting Products & States of Matter for DOUBLE REPLACEMENT REACTIONS
Tips to remember:
AX + BY 
Metals (+) always come first!
Criss-cross to get subscripts.
Deal with number problems by balancing at the end.
Video Example 2:
Potassium chromate and silver nitrate
Reactant formulas:
K2CrO4 + AgNO3  [TIP: Label each element with its charge]
Unbalanced Equation:
K2CrO4 + AgNO3  KNO3 + Ag2CrO4
Let’s add states of matter.

20. Last Question on Note-taking Guide
DOUBLE REPLACEMENT EXAMPLE:
Zinc chloride + ammonium sulfide 
Reactant formulas:
ZnCl2 + (NH4)2S 
Unbalanced equation:
ZnCl2 + (NH4)2S  ZnS + NH4Cl
Balanced equation:
ZnCl2 + (NH4)2S  ZnS + 2NH4Cl
Let’s add states of matter.

21. As you come in, Materials: Practice packet
Predicting Products note-taking guide
Discovering the Indicators of a Reaction lab
Plan:
Types of Reactions Quiz (TIME LIMIT: 15 minutes)
Predicting Products of Single Replacement & finish lab
Learn to write Net Ionic Equations
Tonight:
Practice predicting products and balancing equations for tomorrow’s quiz!
Read over the Student Learning Activities. Have you been working the suggested problems in your practice packet?

22. Let’s add states of matter.
Predicting Products & States of Matter for SINGLE REPLACEMENT REACTIONS
Tips to remember:
A + BX  CONSULT ACTIVITY SERIES TO BEGIN!
Metals (+) always come first in a compound!
Lone metals replace compound metals or hydrogen.
Lone nonmetals replace compound nonmetals.
Criss-cross to get subscripts.
Deal with number problems by balancing at the end.
Example:
Potassium and silver nitrate
Reactant formulas:
K + AgNO3  [TIP: Label each element with its charge]
Unbalanced Equation:
K + AgNO3  KNO3 + Ag
Let’s add states of matter.

23. Predicting Products & States of Matter SINGLE REPLACEMENT
“Long Worksheet” example
52. Al + HCl 
Who will Al try to replace?
Is Al more active than H?
Criss-cross to write the products. Look for diatomic elements!
Unbalanced Equation: Al + HCl  AlCl3 + H2
Balanced Equation: 2Al + 6HCl  2AlCl3 + 3H2
Let’s add states of matter.

24. DISCOVERING INDICATORS OF A CHEMICAL REACTION LAB
For each reaction:
Predict the Products.
Write a balanced equation.
List as many observations as possible during the reaction.

25. Reactions in Aqueous Solution
MANY reactions occur in water:
More than 70% of earth is covered by water
66% of the human body is water
Many ionic compounds dissociate in water. They are described as (aq) in reactions.
Often aqueous reactions form solids called precipitates

26. Net Ionic Equations
Purpose: Communicate the real action of the reaction and leave out the insignificant ions/elements
Begin with a balanced equation and states of matter.
Write a complete ionic equation, taking apart all aqueous compounds.
Remove spectator ions
Leaves a balanced net ionic equation
Example: Potassium iodide and lead (II) nitrate
Discovering the Indicators of a Reaction: Station 2

27. Why do I set up the lab with so many aqueous solutions?
Rate of Reaction
Temperature – warmer = faster reaction; particles are moving faster
Concentration - # of particles; more particles = faster reaction
State of Matter – dissolved means greater surface area; more surface area = faster reaction
Surface Area - Filings, shot, powder, mossy, etc.; greater surface area = faster reaction
Catalyst – DOES NOT REACT; lowers the activation energy of the reaction

28. Predicting Products & States of Matter
52. 2Al(s) + 6HCl(aq)  2AlCl3(aq) + 3H2(g)
56.ZnCl2 + (NH4)2S  2NH4Cl + ZnS

29. Predicting Products & States of Matter
56.ZnCl2 (aq)+ (NH4)2S(aq)  2NH4Cl(aq) + ZnS(s)
59. HgSO4 + 2NH4NO3  Hg(NO3)2 + (NH4)2SO4

30. Predicting Products & States of Matter
59. HgSO4(aq) + 2NH4NO3(aq)  Hg(NO3)2(aq) + (NH4)2SO4(aq)
60. Fe + CuSO4  FeSO4 + Cu

31. Predicting Products & States of Matter
60. Fe (s)+ CuSO4 (aq)  FeSO4 (aq) + Cu (s)
67. Br2 + 2NaI  2NaBr + I2

32. Predicting Products & States of Matter
67. Br2 (l) + 2NaI(aq)  2NaBr (aq) + I2 (g)

33. Evidence of a Chemical Reaction
Formation of a gas
Bubbles
Smell
Formation of a solid (precipitate) from two aqueous solutions; often solids are colorful
“Snow globe” effect
“Paint” look
“Jello” consistency
Change in temperature
Test tube feels colder to you (endothermic reaction)
Test tube feels warmer to you (exothermic reaction)
Produces light

34. Colored Pencil Corrections
Al(NO3)3 + NaOH = Al(OH)3 + NaNO3
KClO3 = KCl + O2
H3PO4 + Mg(OH)2 = Mg3(PO4)2 + H2O
NH4NO2 = N2 + H2O
BaCl2 + Na2SO4 = NaCl + BaSO4
Fe2O3 + CO = Fe + CO2
Mg(OH)2 + (NH4)3PO4 = Mg3(PO4)2 + NH3 + H2O