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5. Describe and identify five general types of reactions.
6. Write equations for the five general types of reactions.
7. Predict the products of the five general types of reactions. Slide
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11.2
Types of Chemical Reactions
The heat and smoke of burning
charcoal are the products of a
combustion reaction.
Combustion is one of the five
general types of chemical
reactions. If you can recognize
a reaction as being a particular
type, you may be able to
predict the products of the
reaction.
© Copyright Pearson Prentice Hall
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• Balancing chemical equations:
1. Determine correct formulas of reactants and products and write skeleton equation
2. Count numbers of atoms of each element on each side of arrow (count polyatomic ion as a unit)
3. Change coefficients until the equation balances
4. Check each atom or polyatomic ion to make sure it is balanced
5. Make sure coefficients are in lowest possible ratio
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• Types of Reactions: 5 general categories
1.
2.
3.
4.
5.
Combination
Decomposition
Single replacement
Double replacement
Combustion
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1. Combination Reactions
– Two or more substances combine to form a single product
– General formula: R + S → RS
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• Practice: Write the balanced equation for a combination reaction:
Mg + O2 →
– First complete the skeleton equation:
Mg + O2 → MgO
– Then balance:
2Mg + O2 → 2MgO
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11.2
Types of Chemical Reactions
>
Classifying Reactions
Combination Reactions
A combination reaction is a chemical change
in which two or more substances react to form a
single new substance.
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© Copyright Pearson Prentice Hall
• Write and balance this combination reaction: P + O2 → tetraphosphorus decoxide
1. Write skeleton equation:
P + O2 → P4O10
2. Then balance
4P + 5O2 → P4O10
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N2O5 + H2O → nitric acid
• Finish and balance this combination reaction:
1. Write skeleton equation:
N2O5 + H2O → HNO3
2. Then balance
N2O5 + H2O → 2HNO3
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Fe + O2 → iron(II) oxide
1. First write skeleton equation:
Fe + O2 → FeO
2. Then balance:
2Fe + O2 → 2FeO
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2. Decomposition Reactions
– A single compound is broken down into two or more products
– Most require energy: heat, light or electricity
– General formula: RS → R + S
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11.2
Types of Chemical Reactions
>
Classifying Reactions
A decomposition reaction is a chemical change
in which a single compound breaks down into two
or more simpler products.
When orangecolored mercury(II)
oxide is heated, it
decomposes into
its constituent
elements: liquid
mercury and
gaseous oxygen.
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© Copyright Pearson Prentice Hall
• Predict the binary compound that will decompose to form: H2 + Br2
HBr
• Write the balanced equation:
2HBr → H2 + Br2
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• Write the balanced equation for the decomposition reaction:
Ag2O →
Write skeleton equations
Ag2O → Ag + O2
Then balance:
2Ag2O → 4Ag + O2
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• Write the balanced chemical equation showing the decomposition of water into its elements.
2H2O → 2H2 + O2
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• What is the balanced equation for the following reaction?
nickel(II)carbonate → nickel(II)oxide + ?
• First write the correct formulas:
NiCO3 → NiO + • Then try and predict the other compound:
NiCO3 → NiO + CO2
• Then balance
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• Qs 13‐15, pg 331‐2
• Q’s 44‐47 pg. 347
• Read pg. 333‐341
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