Types of Chemical Reactions

Study Notes

Synthesis Reactions: Two or more substances combine to form a new compound.
- Example: 2H2 + O2 → 2H2O
Decomposition Reactions: A single compound breaks down into two or more substances.
- Example: 2H2O → 2H2 + O2
Replacement Reactions: One element replaces another element in a compound.
- Example: Zn + CuSO4 → ZnSO4 + Cu
Combustion Reactions: A substance reacts with oxygen to produce heat and light.
- Example: 2CH4 + 3O2 → 2CO2 + 3H2O
Neutralization Reactions: An acid reacts with a base to produce a salt and water.
- Example: HCl + NaOH → NaCl + H2O

Chemical Equations: A symbolic representation of a chemical reaction, using formulas and arrows to indicate the reactants and products.
Reactants: The substances that undergo a chemical change.
Products: The substances formed as a result of a chemical reaction.
Activation Energy: The minimum energy required for a chemical reaction to occur.
Catalysts: Substances that speed up a chemical reaction without being consumed or altered.

Concentration: Increasing the concentration of reactants can increase the rate of reaction.
Temperature: Increasing the temperature can increase the rate of reaction.
Surface Area: Increasing the surface area of reactants can increase the rate of reaction.
Pressure: Increasing the pressure can increase the rate of reaction.
Catalysts: The presence of catalysts can increase the rate of reaction.

Rate of Reaction: The speed at which a chemical reaction occurs.
Collision Theory: The theory that chemical reactions occur when particles collide with sufficient energy.
Factors Affecting Rate: Concentration, temperature, surface area, pressure, and catalysts can affect the rate of reaction.
Rate-Determining Step: The slowest step in a chemical reaction, which determines the overall rate.

Synthesis reactions combine two or more substances to form a new compound, e.g., 2H2 + O2 → 2H2O.
Decomposition reactions involve a single compound breaking down into two or more substances, e.g., 2H2O → 2H2 + O2.
Replacement reactions occur when one element replaces another element in a compound, e.g., Zn + CuSO4 → ZnSO4 + Cu.
Combustion reactions involve a substance reacting with oxygen to produce heat and light, e.g., 2CH4 + 3O2 → 2CO2 + 3H2O.
Neutralization reactions occur when an acid reacts with a base to produce a salt and water, e.g., HCl + NaOH → NaCl + H2O.

Chemical equations symbolically represent a chemical reaction, using formulas and arrows to indicate reactants and products.
Reactants are substances that undergo a chemical change.
Products are substances formed as a result of a chemical reaction.
Activation energy is the minimum energy required for a chemical reaction to occur.
Catalysts are substances that speed up a chemical reaction without being consumed or altered.

Rate of reaction is the speed at which a chemical reaction occurs.
Collision theory states that chemical reactions occur when particles collide with sufficient energy.
Factors affecting the rate of reaction include concentration, temperature, surface area, pressure, and catalysts.
The rate-determining step is the slowest step in a chemical reaction, which determines the overall rate.