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Types of Reactions
Including reaction prediction
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Generals about writing Equations
Generals about writing Equations
Reactants on the left and products on the right
Symbols - see text for symbols that are included in equations.Ex: g for gas, l for liquid, s for solidDownward arrow for precipitate, aq for aqueous
Catalyst goes above the arrow KI
Ex H2O2(aq) ---> H2O(l) + O2(g)
Diatomic Molecules - BrINClHOFElemental state - Br2I2N2Cl2H2O2F2
Reactants on the left and products on the right
Symbols - see text for symbols that are included in equations.Ex: g for gas, l for liquid, s for solidDownward arrow for precipitate, aq for aqueous
Catalyst goes above the arrow KI
Ex H2O2(aq) ---> H2O(l) + O2(g)
Diatomic Molecules - BrINClHOFElemental state - Br2I2N2Cl2H2O2F2
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1. Synthesis (Combination)1. Synthesis (Combination)
Two or more substances react to form a single substance
R + S --> RSEx) SO3(g) + H2O(l) --> H2SO4(aq) Usually gives off energy when forming
bondsExample: Write the balanced equation for:
magnesium ribbon reacting with oxygenMg(s) + O2(g) ---> MgO(s)
2 Mg(s) + O2(g) --> 2MgO(s)
Two or more substances react to form a single substance
R + S --> RSEx) SO3(g) + H2O(l) --> H2SO4(aq) Usually gives off energy when forming
bondsExample: Write the balanced equation for:
magnesium ribbon reacting with oxygenMg(s) + O2(g) ---> MgO(s)
2 Mg(s) + O2(g) --> 2MgO(s)
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1. Synthesis (Combination)1. Synthesis (Combination)
Your turn. Write balanced equations for the following:Aluminum (s) reacts with oxygen (g)Hydrogen (g) reacts with oxygen (g)
Answers:4 Al(s) + 3 O2 ---> 2 Al2O3(s)
2 H2(g) + O2(g) ---> 2 H2O(l)
Your turn. Write balanced equations for the following:Aluminum (s) reacts with oxygen (g)Hydrogen (g) reacts with oxygen (g)
Answers:4 Al(s) + 3 O2 ---> 2 Al2O3(s)
2 H2(g) + O2(g) ---> 2 H2O(l)
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2. Decomposition2. Decomposition
A single compound is broken down into simpler products
RS --> R + SEx) BCl3 --> B + Cl2Requires energy to break chemical bonds
(heat, light, electricity)Example - Write the balanced equation for
mercury (II) oxide decomposing;HgO --> Hg + O2
2HgO --> 2Hg + O2
A single compound is broken down into simpler products
RS --> R + SEx) BCl3 --> B + Cl2Requires energy to break chemical bonds
(heat, light, electricity)Example - Write the balanced equation for
mercury (II) oxide decomposing;HgO --> Hg + O2
2HgO --> 2Hg + O2
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2. Decomposition2. Decomposition
Your turn. Write balanced equations for the following:
The decomposition of waterThe decomposition of lead (IV) oxideAnswers
2 H2O(l) --> 2 H2(g) + O2(g)
PbO2(s) --> Pb(s) + O2(g)
Your turn. Write balanced equations for the following:
The decomposition of waterThe decomposition of lead (IV) oxideAnswers
2 H2O(l) --> 2 H2(g) + O2(g)
PbO2(s) --> Pb(s) + O2(g)
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3. Single Replacement Reactions
3. Single Replacement Reactions
An element replaces an element of a compound
T + RS --> TS + REx) Zn(s) + H2SO4(aq) --> ZnSO4(aq) + H2(g)
A metal may replace a metal or a nonmetal may replace a nonmetal
Activity Series - list of metal in order of decreasing activity
Nonmetals reactivity decreases as you go down the periodic table
This is limited to the halogens -group 7A
An element replaces an element of a compound
T + RS --> TS + REx) Zn(s) + H2SO4(aq) --> ZnSO4(aq) + H2(g)
A metal may replace a metal or a nonmetal may replace a nonmetal
Activity Series - list of metal in order of decreasing activity
Nonmetals reactivity decreases as you go down the periodic table
This is limited to the halogens -group 7A
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3. Single replacement reactions3. Single replacement reactions
Ex) Write the balanced equation when aluminum reacts with sulfuric acid
Al(s) + H2SO4(aq) --> Al2(SO4)3(s) + H2(g)
2Al(s)+ 3H2SO4(aq) --> Al2(SO4)3(s) + 3H2(g)
Ex) Write the balanced equation when aluminum reacts with sulfuric acid
Al(s) + H2SO4(aq) --> Al2(SO4)3(s) + H2(g)
2Al(s)+ 3H2SO4(aq) --> Al2(SO4)3(s) + 3H2(g)
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3. Single replacement reactions3. Single replacement reactions
Your turn. Write balanced equations for the following:
When chlorine reacts with potassium iodide
When copper (assume Cu2+) is added to Iron (II) Sulfate
Answers Cl2(g) + 2 KI(aq) --> 2 KCl(aq) + I2Cu + FeSO4 --> no reaction (no rxn)
Your turn. Write balanced equations for the following:
When chlorine reacts with potassium iodide
When copper (assume Cu2+) is added to Iron (II) Sulfate
Answers Cl2(g) + 2 KI(aq) --> 2 KCl(aq) + I2Cu + FeSO4 --> no reaction (no rxn)
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4. Double Replacement4. Double Replacement
Exchange of positive ions between two compounds. Just swap the positive ions and write the new formula.
R+S- + T+U- --> R+U- + T+S-
Ex) FeS(s) + 2HCl(aq) --> H2S(g) + FeCl2(aq)
Ex) Write the balanced equation for barium chloride added to potassium carbonate
BaCl2(aq) + K2CO3(aq) --> BaCO3(s) + KCl(aq)
BaCl2(aq) + K2CO3(aq) --> BaCO3(s) + 2 KCl(aq)
Exchange of positive ions between two compounds. Just swap the positive ions and write the new formula.
R+S- + T+U- --> R+U- + T+S-
Ex) FeS(s) + 2HCl(aq) --> H2S(g) + FeCl2(aq)
Ex) Write the balanced equation for barium chloride added to potassium carbonate
BaCl2(aq) + K2CO3(aq) --> BaCO3(s) + KCl(aq)
BaCl2(aq) + K2CO3(aq) --> BaCO3(s) + 2 KCl(aq)
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4. Double Replacement4. Double Replacement
Your turn. Write balanced equations for the following.
Iron (III) Sulfide reacting with hydrochloric acid
AnswerFe2S3(s)+ 6 HCl(aq) --> 2 FeCl3(aq) + 3
H2S(g)
Your turn. Write balanced equations for the following.
Iron (III) Sulfide reacting with hydrochloric acid
AnswerFe2S3(s)+ 6 HCl(aq) --> 2 FeCl3(aq) + 3
H2S(g)
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5. Combustion Reactions5. Combustion Reactions
Oxygen reacts with another substance, often producing heat and light
Often involve hydrocarbons Compounds of hydrogen and carbon
Combustion of hydrocarbons produces a lot of energy, therefore, hydrocarbons are used as fuels.
Examples: methane, propane, butane, octane
Oxygen reacts with another substance, often producing heat and light
Often involve hydrocarbons Compounds of hydrogen and carbon
Combustion of hydrocarbons produces a lot of energy, therefore, hydrocarbons are used as fuels.
Examples: methane, propane, butane, octane
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5. Combustion Reactions5. Combustion Reactions
Two types of combustion1. Complete combustionCxHy + O2(g) --> CO2(g) + H2O(g) +
energy2. Incomplete combustionTwo more products: CO and C CxHy + O2(g) --> CO2(g) + H2O(g) + CO(g) + C(s) +
energy
Two types of combustion1. Complete combustionCxHy + O2(g) --> CO2(g) + H2O(g) +
energy2. Incomplete combustionTwo more products: CO and C CxHy + O2(g) --> CO2(g) + H2O(g) + CO(g) + C(s) +
energy
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5. Combustion Reactions5. Combustion Reactions
Ex) Write a balanced equation for the complete combustion of C3H8.
C3H8(g) + O2(g) --> CO2(g) + H2O(g) + energy C3H8(g) + 5 O2(g) --> 3 CO2(g) + 4H2O(g) + energy
Your turn: Write a balanced equation for the complete combustion of C8H18.
Answer2 C3H18(l) + 25 O2(g) --> 16 CO2(g) + 18 H2O(g) +
energy
Ex) Write a balanced equation for the complete combustion of C3H8.
C3H8(g) + O2(g) --> CO2(g) + H2O(g) + energy C3H8(g) + 5 O2(g) --> 3 CO2(g) + 4H2O(g) + energy
Your turn: Write a balanced equation for the complete combustion of C8H18.
Answer2 C3H18(l) + 25 O2(g) --> 16 CO2(g) + 18 H2O(g) +
energy
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