Chemical Reactions Types

Study Notes

A chemical reaction is a process in which one or more substances are converted into new substances.
Chemical reactions involve the transformation of reactants into products.

Synthesis Reaction: A reaction in which two or more substances combine to form a new compound.
- Example: 2H2 + O2 → 2H2O
Decomposition Reaction: A reaction in which a single compound breaks down into two or more simpler substances.
- Example: 2H2O → 2H2 + O2
Single Displacement Reaction: A reaction in which one element displaces another element from a compound.
- Example: Zn + CuSO4 → ZnSO4 + Cu
Double Displacement Reaction: A reaction in which two compounds exchange partners, resulting in the formation of two new compounds.
- Example: NaCl + AgNO3 → NaNO3 + AgCl
Combustion Reaction: A reaction in which a substance reacts with oxygen to produce heat and light.
- Example: 2CH4 + 3O2 → 2CO2 + 3H2O

A chemical equation is a representation of a chemical reaction using chemical formulas and symbols.
Chemical equations must be balanced, meaning the number of atoms of each element must be the same on both the reactant and product sides.

Reactants: The substances that undergo a chemical change in a reaction.
Products: The substances formed as a result of a chemical reaction.
Arrow: Represented by →, indicates the direction of the reaction.
Coefficients: Numbers placed in front of formulas of reactants or products to balance the equation.
States of Matter: Indicated by (s) for solid, (l) for liquid, (g) for gas, and (aq) for aqueous solution.

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 atoms of each element on both sides.
3. Add coefficients to balance the equation.
4. Check the equation to ensure it is balanced.

A chemical reaction is a process that converts one or more substances into new substances.

Synthesis Reaction: Two or more substances combine to form a new compound, e.g., 2H2 + O2 → 2H2O.
Decomposition Reaction: A single compound breaks down into two or more simpler substances, 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, forming 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.

A chemical equation represents a chemical reaction using chemical formulas and symbols.
Chemical equations must be balanced, ensuring the number of atoms of each element is the same on both the reactant and product sides.

Reactants: Substances that undergo a chemical change in a reaction.
Products: Substances formed as a result of a chemical reaction.
Arrow: Represented by →, indicating the direction of the reaction.
Coefficients: Numbers placed in front of formulas of reactants or products to balance the equation.
States of Matter: Indicated by (s) for solid, (l) for liquid, (g) for gas, and (aq) for aqueous solution.

Law of Conservation of Mass: Matter cannot be created or destroyed in a chemical reaction.
Balancing Steps:
- Write the unbalanced equation.
- Count the atoms of each element on both sides.
- Add coefficients to balance the equation.
- Check the equation to ensure it is balanced.