1. Combination Reactions (Synthesis Reactions)
* General Equation: A + B → AB
* Description: Two or more reactants combine to form a single product.
* Example: 2Na (s) + Cl₂ (g) → 2NaCl (s) (Sodium and chlorine gas react to form sodium chloride)
2. Decomposition Reactions
* General Equation: AB → A + B
* Description: A single reactant breaks down into two or more products.
* Example: 2H₂O (l) → 2H₂ (g) + O₂ (g) (Water decomposes into hydrogen and oxygen gas)
3. Single Displacement Reactions
* General Equation: A + BC → AC + B
* Description: One element replaces another in a compound.
* Example: Zn (s) + CuSO₄ (aq) → ZnSO₄ (aq) + Cu (s) (Zinc replaces copper in copper sulfate)
4. Double Displacement Reactions
* General Equation: AB + CD → AD + CB
* Description: Two compounds exchange ions to form two new compounds.
* Example: AgNO₃ (aq) + NaCl (aq) → AgCl (s) + NaNO₃ (aq) (Silver nitrate and sodium chloride react to form silver chloride and sodium nitrate)
5. Combustion Reactions
* General Equation: Fuel + Oxidant → Products (usually CO₂ and H₂O)
* Description: A substance rapidly reacts with an oxidant (usually oxygen) to produce heat and light.
* Example: CH₄ (g) + 2O₂ (g) → CO₂ (g) + 2H₂O (g) (Methane burns in oxygen to produce carbon dioxide and water)
Note: These are the most common types of reactions. There are other classifications, like neutralization reactions (acid-base) and redox reactions, which involve electron transfer.
