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11/29/07
Complete the following single replacement reaction:
Zn + HCl 
Complete the following double replacement reaction:
NaCl + K2SO4 
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Hindenburg
on May 6, 1937, the Hindenburg carrying 61 crew and 36 passengers arrived hours behind schedule at Lakehurst Naval Air Station in New Jersey.
36 people passed away
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3. Chapter 8
Types of Reactions

4. Indicators of a Chemical Reaction
Evolution of heat and light
Production of Gas
Formation of Precipitate
Solid formed as a result of a chemical reaction
Color Change
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5. Examples of Each Indicator
Ammonium Dichromate Decomposition
ammonium dichromate
(NH4)2Cr2O7(s)    Cr2O3(s)  +  N2(g)  +  4H2O(g)
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Production of a Gas
Remember in grade school, our volcano project
Vinegar (acetic acid) + baking soda
HC2H3O2 + NaHCO3 ===> NaC2H3O2 + H2CO3
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7. Formation of Precipitate/Color
Pb(NO3)2(aq) + 2 KI(aq) --> PbI2(s) + 2 KNO3(aq)
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8. Types of Chemical Reactions
Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion
Acid-Base Reaction
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Many chemical reactions have defining characteristics which allow them to be classified.
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Synthesis Reactions
Two or more substances combine to form one substance.
The general form is A + X AX
Example:
Magnesium + oxygen  magnesium oxide
2Mg + O2  2MgO
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Synthesis Reactions
Synthesis reactions may also be called composition or combination reactions.
Types of synthesis reactions:
Combination of elements
K + Cl2 
One product will be formed
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Synthesis Reactions
K + Cl2 
Write the ions: K+ Cl-
Balance the charges: KCl
Balance the equation: 2K + Cl2  2KCl
Remember those elements that are diatomic !
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Synthesis Reactions
Some types of synthesis reactions:
Oxide + water 
Nonmetal oxide + water  acid
SO2 + H2O  H2SO3
Metal oxide + water  base
BaO + H2O  Ba(OH)2
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Synthesis Reactions
Some types of synthesis reactions:
Metal oxides + nonmetal oxides
Na2O + CO2  Na2CO3
CaO + SO2  CaSO3
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15. Decomposition Reactions
One substance reacts to form two or more substances.
The general form is AX  A + X
Example:
Water can be decomposed by electrolysis.
2H2O  2H2 + O2
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16. Passing water through a current will release hydrogen and oxygen.
Electrolysis of Water
electricity
2H2O(l) ---- 2H2 (g) + O2(g)
Passing water through a current will release hydrogen and oxygen.
The decomposition of a substance by an electric current is called electrolysis.
Airbags deploy through a decomposition reaction
Sodium Azide
2NaN3  Na3N + 4N2
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17. Decomposition Reactions
Types of Decomposition Reactions:
Decomposition of carbonates
When heated, some carbonates break down to form an oxide and carbon dioxide.
CaCO3  CaO + CO2
H2CO3  H2O + CO2
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18. Decomposition Reactions
Types of decomposition reactions:
Some metal hydroxides decompose into oxides and water when heated.
Ca(OH)2  CaO + H2O
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19. Decomposition Reactions
Types of decomposition reactions:
Metal chlorates decompose into chlorides and oxygen when heated.
2KClO3  2KCl + 3O2
Zn(ClO3)2  ZnCl2 + 3O2
Some of these reactions are used in explosives.
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20. Single Replacement Reactions
A metal will replace a metal ion in a compound.
The general form is A + BX  AX + B
A nonmetal will replace a nonmetal ion in a compound.
The general form is Y + BX  BY + X
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21. Single Replacement Reactions
Examples:
Ni + AgNO3 
Nickel replaces the metallic ion Ag+.
The silver becomes free silver and the nickel becomes the nickel(II) ion.
Ni + AgNO3  Ag + Ni(NO3)2
Balance the equation:
Ni + 2AgNO3  2Ag + Ni(NO3)2
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22. Single Replacement Reactions
Not all single replacement reactions that can be written actually happen.
The metal must be more active than the metal ion.
We determine whether the reaction can occur or not through the use of the activity series.
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Element’s activity--ability of an element to react
Activity series--list of elements that are organized according by their ease to undergo chemical rxns
Metals:
Ease to lose electrons (form cations)
Nonmetals
Ease to gain electrons (form anions)
Order is determined mainly by single replacement rxns
Activity series is used to predict if a reaction will happen or not
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24. Example of Single Replacement
Copper reacts in silver nitrate
Cu + AgNO3CuNO3 + Ag
Grows gray fur (silver) on a penny)
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Practice
Ni + CuCl2 
Zn + Pb(NO3)2 
Cl2 + KI -
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26. Double Replacement Reactions
Ions of two compounds exchange places with each other.
The general form is
AX + BY  AY + BX
Switch partners
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27. Double Replacement Reactions
Think about it like “foil” in algebra, first and last ions go together + inside ions go together
Example:
AgNO3(aq) + NaCl(s)  AgCl(s) + NaNO3(aq)
Another example:
K2SO4(aq) + Ba(NO3)2(aq)  KNO3(aq) + BaSO4(s) 2
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Practice
Predict the products. Balance the equation
HCl(aq) + AgNO3(aq) 
CaCl2(aq) + Na3PO4(aq) 
Pb(NO3)2(aq) + BaCl2(aq) 
FeCl3(aq) + NaOH(aq) 
H2SO4(aq) + NaOH(aq) 
KOH(aq) + CuSO4(aq) 
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5. Combustion Reactions
occur when a hydrocarbon reacts with oxygen gas.
This is also called burning!!! In order to burn something you need the 3 things in the “fire triangle”: 1) A Fuel (hydrocarbon) 2) Oxygen to burn it with 3) Something to ignite the reaction (spark)
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Combustion Reaction
Methane, CH4, is natural gas.
When hydrocarbon compounds are burned in oxygen, the products are water and carbon dioxide.
CH4 + O2  CO2 + H2O
CH4 + 2O2  CO2 + 2H2O
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Combustion Reactions
In general: CxHy + O2  CO2 + H2O
Products in combustion are ALWAYS carbon dioxide and water. (although incomplete burning does cause some by-products like carbon monoxide)
Combustion is used to heat homes and run automobiles (octane, as in gasoline, is C8H18)
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Combustion Reactions
Edgar Allen Poe’s drooping eyes and mouth are potential signs of CO poisoning.
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Combustion
Example
C5H O2  CO2 + H2O
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Acid-base reactions:
Anytime you have an acid or base as a reactant and a salt is formed:
NH4OH + HCl  NH4Cl2 + 2H2O (Space shuttle)
Antacids
Ca(OH) HCl  CaCl2 + 2H2O
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35. Steps to Writing Reactions
Some steps for doing reactions
Identify the type of reaction
Predict the product(s) using the type of reaction as a model
Balance it
Don’t forget about the diatomic elements! (BrINClHOF) For example, Oxygen is O2 as an element.
In a compound, it can’t be a diatomic element because it’s not an element anymore, it’s a compound!
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36. Review of Balancing Chemical Reactions
Use MNOH
First balance metals
Then nonmetals
Then Oxygen
Then Hydrogen
Remember you only can change the coefficients, not the subscripts
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37. Use of Symbols in Reactions see page 246
aq (aqueous) in water
s (solid)
l (liquid)
Delta (when heated)
 (yields)
Gas
reversible reaction
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Classify each of the following as to type:
H2 + Cl2  2HCl
Synthesis
Ca + 2H2O  Ca(OH)2 + H2
Single replacement
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Practice
CH4 + O2  CO2 + H2O
Combustion
2KClO3  2KCl + 3O2
Decomposition
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Practice
FeS + 2HCl  FeCl2 + H2S
Double replacement
Zn + HCl  ?
Single replacement
Zn + 2HCl  ZnCl2 + H2
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Mixed Practice
State the type, predict the products, and balance the following reactions:
BaCl2 + H2SO4 
C6H12 + O2 
Zn + CuSO4 
Cs + Br2 
FeCO3 
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42. Types of Chemical Reactions
Read Chapter 8
Review nomenclature and ions
Do all of the practice exercises given in class.
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