As you come in,

1
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.

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

1. Zn Pb(NO3)2 --gt Zn(NO3)2 Pb
2. 2 AlBr3 3 Cl2 --gt 2 AlCl3 3 Br2
3. 2 Na3PO4 3 CaCl2 --gt Ca3(PO4)2 6 NaCl
4. 2 K Cl2 --gt 2 KCl
5. 2 Al 6 HCl --gt 2 AlCl3 3 H2
6. 3 Ca(OH)2 2 H3PO4 --gt Ca3(PO4)2 6 H2O
7. Cu 2 H2SO4 --gt CuSO4 2 H2O SO2
8. 2 H2 2 NO --gt 2 H2O N2

9
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 tomorrows quiz
• Tonight
• Go to Edmodo.
• DUE TOMORROW Predicting Products note-taking
  guide
• Practice balancing equations for tomorrows quiz!

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

1. Zn Pb(NO3)2 --gt Zn(NO3)2 Pb
2. 2KClO3 ? 2KCl 3 O2
3. 2 AlBr3 3 Cl2 --gt 2 AlCl3 3 Br2
4. 2 Na3PO4 3 CaCl2 --gt Ca3(PO4)2 6 NaCl
5. 2 K Cl2 --gt 2 KCl
6. 2 Al 6 HCl --gt 2 AlCl3 3 H2
7. CH4 2O2 ? CO2 2H2O
8. 3 Ca(OH)2 2 H3PO4 --gt Ca3(PO4)2 6 H2O

13
Single Replacement ReactionsSPECIAL! MORE TO
COME!

• A BX --gt 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
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
  Mondays 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
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

Lets 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

Lets 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 tomorrows quiz!
• Read over the Student Learning Activities. Have
  you been working the suggested problems in your
  practice packet?

22
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

Lets add states of matter.
23
Predicting Products States of MatterSINGLE
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

Lets 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