1. 8.3 – NOTES Decomposition

2. C. Decomposition reactions a single compound breaks down to produce two or more products
usually requires heat, light, or electricity; air bags inflating is a result of a decomposition reaction (sodium azide)
difference b/t heating and burning – heating does not require oxygen, but burning does

3. 1. Metallic chlorates will produce metal chlorides and oxygen gas;
2 NaClO3  2 NaCl + 3 O2
Ga(ClO3)3  GaCl O2

4. 2. Carbonates will produce a metal oxide and carbon dioxide;
PbCO3  PbO + CO2
Al2(CO3)3  Al2O3 + 3 CO2

5. 3. Metallic hydroxides will produce a metal oxide and water vapor
2 LiOH  Li2O + H2O
Ti(OH)4  TiO2 + 2 H2O

6. 4. Certain acids will produce a nonmetallic oxide and water; these are the only two Chem I is responsible for knowing; acids are aqueous
Carbonic acid
H2CO3  H2O + CO2
Sulfurous acid
H2SO3  H2O + SO2

7. 5. Certain metal oxides will produce the elements; metal must be an inactive metal or one with a low reactivity; Au, Ag, Pt, etc.; metal oxides are usually solid
2HgO  2Hg + O2
2Au2O3  4Au + 3O2

8. 6. Electrolysis of molten salts will produce the elements; molten means liquid
Molten LiBr: 2LiBr  2Li + Br2
CaCl2  Ca + Cl2