1. Chapter 5 Section 2 Notes
Reaction Types

2. Synthesis Reaction
Synthesis Reaction: a reaction in which at least 2 substances make a new, more complex compound.
General Form: A + B → AB
Example: 2Na + Cl2 → 2NaCl

3. Synthesis Reaction

4. Decomposition Reaction
Decomposition Reaction: a reaction in which one compound breaks into at least 2 parts
General Form: AB → A + B
Example: 2H2O → 2H2 + 02
Electrolysis: the decomposition of a compound by electric current.

5. Decomposition Reaction

6. Combustion Reaction
Combustion Reaction: a reaction in which a compound and oxygen burn.
Note: carbon containing compound & oxygen are always reactants and carbon dioxide & water are always products.
If the air supply is limited when carbon-containing fuel burns, there might not be enough oxygen gas for all of the carbon to form carbon dioxide. In that case, carbon monoxide may form. Carbon monoxide is dangerous because it has no color or odor and you can’t tell when it’s present.

7. Combustion Reaction

8. Single-Displacement Reaction
Single-Displacement Reaction: A reaction in which the atoms of one element take the place of atoms of another element in a compound.
General Form: XA + B → BA + X

9. Single-Displacement Reaction
Note: Generally, a more reactive element will take the place of a less reactive one.
Example:
3CuCl2 + 2Al → 2AlCl3 + 3Cu

10. Single-Displacement Reaction

11. Double-Displacement Reaction
Double-Displacement reaction: a reaction in which a new substance is made by the exchange of ions between 2 compounds.
General Form:
AX + BY → AY + BX
Example:
Pb(NO3)2 + K2CrO4 → PbCrO4 + 2KNO3

12. Double-Displacement Reaction