1. Types of Chemical Reactions

2. 121.Synthesis when two or more elements combine to form a compound.
A + B → AB
Example:
8 Fe + S8 → 8 FeS

3. 122. Decomposition
a compound breaks down to make simpler ones.
AB → A + B
Example:
2 H2O → 2 H2 + O2

4. 123. Single replacement
An element trades places with another element in a compound.
A + BC → AC + B
Example:
Mg +2 HCl→ MgCl2 + H2

5. 124. Double replacement
two elements switch places, forming two new compounds.
AB + CD → AD + CB
Example:
PbBr2 + 2 KCl → PbCl2 + 2 KBr

6. 125. Combustion
when oxygen combines with another compound to form water and carbon dioxide.
These reactions require oxygen.
CH + O2 → CO2 + H2O
Example:
C10H O2 → 10 CO2 + 4 H2O

7. 126. Neutralization or acid/base
when an acid and base react with each other causing the formation of water. H A + B OH ---> H2O + BA Example: HBr + NaOH ---> NaBr + H2O

8. Identify the following chemical equations by type.
C4H8 + 6O2 ---> 4CO2 + 4H2O _______ HCl + NaOH ---> H2O + NaCl _______ 2KNO3 ---> 2KNO2 + O2 _______ AgNO3 + NaCl ---> NaNO3 + AgCl _______ 2Mg + O2 ---> 2MgO _______ MgCO3 ---> MgO + CO2 _______ Cl2 + 2KBr ---> 2KCl + Br2 _______ 2Ag + S ---> Ag2S _______
Double replacement
Combustion
Single replacement
Synthesis
Neutralization
Decomposition