Types of Reactions – Part I
1. Synthesis Reactions
• Formation of new product
Different Conditions
• Element + Element → Compound
o Ex. N2(g) + O2(g) → 2NO(g)
• Element + Compound → More complex compound
o Ex. PCl3(l) + Cl2(g) → PCl5(s)
• Compound + Compound → More complex compound
o I. A Non-metal Oxide Reacting with Water → Acid
o Ex. CO2(g) + H2O(l) → H2CO3(aq)
o II. A Metal Oxide Reacting with Water → Base
o Ex. Na2O(s) + H2O(l) → 2NaOH(aq)
2. Decomposition Reactions
• Breakdown of a molecule into simpler components
Different Conditions
• Binary Compound → Element + Element
o Ex. 2NO(g) → N2(g) + O2(g)
• Metal Nitrate → Metal Nitrite + Oxygen Gas
o Ex. 2NaNO3(s) → 2NaNO2(s) + O2(g)
• Metal Carbonate → Metal Oxide + Carbon Dioxide
o Ex. CaCO3(s) → CaO(s) + CO2(g)
• Metal Hydroxide → Metal Oxide + Water
o Ex. Ca(OH)2(s) → CaO(s) + H2O(l)
3. Combustion Reactions
• The reaction of a substance with oxygen to produce oxides and
energy
A) Complete Combustion
• Burning of a hydrocarbon (Only H & C) to form only water and
carbon dioxide
Ex. CH4 (g) + O2 (g) → CO2 (g) + 2H2O (g)
• Other substances undergo complete combustion to form stable
oxides.
Ex. Mg (s) + O→ MgO(s)
B) Incomplete Combustion
• Burning of a hydrocarbon to form carbon dioxide, water along with
carbon monoxide and carbon (caused by insufficient oxygen).
4CH4 (g) + 6O2 (g) → C
(s)
+ 2CO
(g)
+ CO2 (g) + 8H2O
(g)
Practice! For each of the chemical reactions, predict the products and
balance the chemical equation:
a)
K+
Br2 →
b)
SO3(g) +
c)
Ni2O3 →
d)
LiNO3(s)→
e)
C3H8 + O2 →
(complete)
f)
C3H8 + O2 →
(incomplete)
H2O(l) →