As you come in,
 Materials:
 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.
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

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.
Writing Chemical Equations
Video Example 1:
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
Combustion of H2 gas
• Description: Hydrogen
gas burns in oxygen gas
to produce water vapor.
• Unbalanced equation:
Video Example 2:
Combustion of methane gas
• Description: Methane
gas burns in oxygen gas
to produce carbon
dioxide and water vapor.
• Unbalanced equation:
Balancing Chemical Equations
 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 1:
Combustion of H2 gas
• Unbalanced equation:
H2 + O2  H2O
• Balanced equation:
Video Example 2:
Combustion of methane gas
• Unbalanced equation:
CH4 + O2  CO2 + H2O
• Balanced equation:
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
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.
Writing & Balancing Equations
1.
2.
3.
4.
5.
6.
7.
8.
Zn + Pb(NO3)2 --> Zn(NO3)2 + Pb
2 AlBr3 + 3 Cl2 --> 2 AlCl3 + 3 Br2
2 Na3PO4 + 3 CaCl2 --> Ca3(PO4)2 + 6 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
a
As you come
in,
 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!

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
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
Identify the Type of Reaction
1.
2.
3.
4.
5.
6.
7.
8.
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)2 + 6 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
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.
“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.
“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.
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!

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)
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
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
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
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?

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
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
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.
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
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
 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
Predicting Products & States of Matter
52. 2Al(s) + 6HCl(aq)  2AlCl3(aq) + 3H2(g)
56.ZnCl2 + (NH4)2S  2NH4Cl + ZnS
Predicting Products & States of Matter
56.ZnCl2 (aq)+ (NH4)2S(aq)  2NH4Cl(aq) + ZnS(s)
59. HgSO4 + 2NH4NO3  Hg(NO3)2 + (NH4)2SO4
Predicting Products & States of Matter
59. HgSO4(aq) + 2NH4NO3(aq)  Hg(NO3)2(aq) +
(NH4)2SO4(aq)
60. Fe + CuSO4  FeSO4 + Cu
Predicting Products & States of Matter
60. Fe (s)+ CuSO4 (aq)  FeSO4 (aq) + Cu (s)
67. Br2 + 2NaI  2NaBr + I2
Predicting Products & States of Matter
67. Br2 (l) + 2NaI(aq)  2NaBr (aq) + I2 (g)
Evidence of a Chemical Reaction
Formation of a gas

Bubbles

Smell
2. Formation of a solid (precipitate) from two aqueous
solutions; often solids are colorful

“Snow globe” effect

“Paint” look

“Jello” consistency
3. Change in temperature

Test tube feels colder to you (endothermic reaction)

Test tube feels warmer to you (exothermic reaction)
4. Produces light
1.
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