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Overview of Chemical Reaction Types
Aug 22, 2024
Lecture Notes: Types of Chemical Reactions
1. Combustion Reaction
Definition
: A reaction where a substance burns, releasing heat energy.
Example
: Octane (found in gasoline) reacts with oxygen to produce CO2 and H2O. Water is typically in vapor form due to high temperatures.
Features
:
Hydrocarbon reacts with oxygen.
Produces carbon dioxide and water.
Generates a lot of heat.
2. Synthesis Reaction (Combination Reaction)
Definition
: Two or more reactants combine to form a more complex product.
Examples
:
Magnesium reacts with oxygen to form Magnesium Oxide.
Magnesium Oxide reacts with CO2 to form Magnesium Carbonate.
Features
:
Elements or compounds combine to form a larger compound.
3. Decomposition Reaction
Definition
: A complex substance breaks down into simpler substances.
Examples
:
Magnesium Carbonate decomposes upon heating to Magnesium Oxide and CO2.
Mercury Oxide decomposes into Mercury and Oxygen upon heating.
Water decomposing into Hydrogen and Oxygen gases with electricity.
General Equation
: AB → A + B.
4. Single Replacement Reaction (Single Displacement)
Definition
: An element replaces another in a compound.
Examples
:
Zinc reacts with Copper Chloride to form Zinc Chloride and Copper.
Bromine reacts with Sodium Iodide to form Sodium Bromide and Iodine.
Iron reacts with HCl to form FeCl2 and H2.
General Equation
: A + BC → AC + B.
Note
: Generally metals replace metals, nonmetals replace nonmetals.
5. Double Replacement Reaction (Double Displacement)
Definition
: Exchange of ions between two compounds.
Types
:
Precipitation Reaction
: Forms an insoluble product.
Example: Silver Nitrate + Sodium Chloride → Silver Chloride (solid) + Sodium Nitrate.
Acid-Base Neutralization
: Forms water and a salt.
Example: HCl + NaOH → NaCl + H2O.
Gas Evolution Reaction
: Produces a gas.
General Equation
: AB + CD → AD + CB.
6. Combustion Reaction Review
Hydrocarbon + O2 → CO2 + H2O.
Redox reactions since there is a transfer of electrons.
Redox Reactions
Combustion and Single Replacement are always redox.
Decomposition & Synthesis
:
If pure elements form compounds or vice versa, it's a redox reaction.
Examples and Classification Quizzes
Decomposition
: Calcium Hydroxide decomposes to Calcium Oxide and Water.
Single Replacement
: Zinc reacts with Nickel Chloride to form Zinc Chloride and Nickel.
Synthesis
: Barium Oxide + CO2 → Barium Carbonate.
Gas Evolution
: Sodium Bicarbonate + HCl → NaCl + H2O + CO2.
Summary
Decomposition
: AB → A + B.
Synthesis
: A + B → AB.
Single Replacement
: A + BC → AC + B.
Double Replacement
: AB + CD → AD + CB.
Combustion
: Hydrocarbon + O2 → CO2 + H2O.
Types of Double Replacement
:
Precipitation
Acid-Base Neutralization
Gas Evolution
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