Types of Chemical Reactions

Types of Chemical Reactions

• Synthesis Reaction: Two or more reactants combine to form a single product.
  • Example: 2H2 + O2 → 2H2O
• Decomposition Reaction: A single reactant breaks down into two or more products.
  • Example: 2H2O → 2H2 + O2
• Single Displacement Reaction: One element displaces another element from a compound.
  • Example: Zn + CuSO4 → ZnSO4 + Cu
• Double Displacement Reaction: Two compounds exchange partners, resulting in two new compounds.
  • Example: NaCl + AgNO3 → NaNO3 + AgCl
• Combustion Reaction: A substance reacts with oxygen to produce heat and light.
  • Example: 2CH4 + 3O2 → 2CO2 + 3H2O
• Neutralization Reaction: An acid reacts with a base to form a salt and water.
  • Example: HCl + NaOH → NaCl + H2O

Oxidation and Reduction

• Oxidation: The loss of one or more electrons by an atom, molecule, or ion.
• Reduction: The gain of one or more electrons by an atom, molecule, or ion.
• Oxidizing Agent: A substance that causes oxidation to occur.
• Reducing Agent: A substance that causes reduction to occur.
• Redox Reaction: A reaction that involves both oxidation and reduction.
  • Example: 2K + Cl2 → 2KCl (K is oxidized, Cl2 is reduced)

Balancing Equations

• Law of Conservation of Mass: Matter cannot be created or destroyed in a chemical reaction.
• Balancing Steps:
  1. Write the unbalanced equation.
  2. Count the number of atoms of each element on both sides.
  3. Add coefficients in front of the formulas of the reactants or products to balance the equation.
  4. Check the equation to ensure it is balanced.
• Tips for Balancing:
  • Balance elements that appear in the greatest number of formulas first.
  • Balance elements that appear in the fewest formulas last.
  • Use coefficients, not subscripts, to balance the equation.
  • Check the equation multiple times to ensure it is balanced.

Types of Chemical Reactions

• Synthesis Reaction: Two or more reactants combine to form a single product, e.g. 2H2 + O2 → 2H2O
• Decomposition Reaction: A single reactant breaks down into two or more products, e.g. 2H2O → 2H2 + O2
• Single Displacement Reaction: One element displaces another element from a compound, e.g. Zn + CuSO4 → ZnSO4 + Cu
• Double Displacement Reaction: Two compounds exchange partners, resulting in two new compounds, e.g. NaCl + AgNO3 → NaNO3 + AgCl
• Combustion Reaction: A substance reacts with oxygen to produce heat and light, e.g. 2CH4 + 3O2 → 2CO2 + 3H2O
• Neutralization Reaction: An acid reacts with a base to form a salt and water, e.g. HCl + NaOH → NaCl + H2O

Oxidation and Reduction

• Oxidation: The loss of one or more electrons by an atom, molecule, or ion
• Reduction: The gain of one or more electrons by an atom, molecule, or ion
• Oxidizing Agent: A substance that causes oxidation to occur
• Reducing Agent: A substance that causes reduction to occur
• Redox Reaction: A reaction that involves both oxidation and reduction, e.g. 2K + Cl2 → 2KCl (K is oxidized, Cl2 is reduced)

Balancing Equations

• Law of Conservation of Mass: Matter cannot be created or destroyed in a chemical reaction
• Balancing Steps:
  • Write the unbalanced equation
  • Count the number of atoms of each element on both sides
  • Add coefficients in front of the formulas of the reactants or products to balance the equation
  • Check the equation to ensure it is balanced
• Tips for Balancing:
  • Balance elements that appear in the greatest number of formulas first
  • Balance elements that appear in the fewest formulas last
  • Use coefficients, not subscripts, to balance the equation
  • Check the equation multiple times to ensure it is balanced