Synthesis - Chemical reaction in which two or more substances react to yield a single product.
Examples of Synthesis
- Formation of binary compound : A + B --> AB
- Metal oxide-water reactions : MO + H2O --> base
- Nonmetal oxide-water reactions : (NM)O + H2O --> acid
Decomposition - A type of chemical reaction in which a single compound breaks down into two or more elements or new compounds.
Examples of Decomposition
- Binary Compounds : AB --> A + B
- Metallic Carbonates : MCO3 --> MO + CO2
- Metallic Hydrogen Carbonates : MHCO3 --> MO + H2O + CO2
- Metallic Hydroxides : MOH --> MO + H2O
- Metallic Chlorates : MCIO3 --> MCI + O2
- Oxyacids Decompose to Nonmetal Oxides and Water : acid --> (NM)O + O2
Single Replacement - Chemical reaction that occurs when the atoms of one element replace the atoms of another element in a compound.
Examples of Single Replacement
- Metal-Metal Replacement : A + BC --> AC + B
- Active Metal Replaces H from Water : M + H2O --> MOH + H2
- Active Metal Replaces H from Acid : M + HX --> MX + H2
- Halide-Halide Replacement : D + BC --> BD + C
Double Replacement - A chemical reaction where two compounds react where the positive ions and the negative ions of the two reactants switch places, forming two new compounds or products.
Examples of Double Replacement
- Formation of a Precipitate from Solution
- Acid-Base Neutralization Reaction
Combustion Reaction - A chemical reaction that occurs when a substance reacts with oxygen releasing energy in the form of heat or light.
Example of Combustion
- Hydrocarbon + Oxygen --> Carbon Dioxide + Water
How to use activity series :
- Find if the metal above the other metal
- If it is, then the metal can replace the metal in a reaction. If not, then the metal can NOT be replaced
How to use solubility rules:
- Read the rules and see which one fits the elements you are using.Decide if element is soluble
- If it is add (ag) to the end of the chemical symbol
- If not, add (s) to the add of the chemical symbol