1.2 Essential Review – Chemical Reactions

Reaction type

Synthesis

Decomposition

Single Displacement

Double Displacement

Combustion

Acid-Base

Description and Example

C7H6O3 + C4H6O3 ⟶ C9H8O4 + C2H4O2
Two or more species react to produce a new reagent (or reagents).

2 H2O2(l) ⟶ 2 H2O(l) + O2(g)
A single reactant breaks down into two or more simple products.

2 HCl(aq) + Zn(s) ⟶ ZnCl2(aq) + H2(g)
One element is replaced by another more reactive element (Example: Redox

Reactions).

AgNO3(aq) + NaCl(aq) ⟶ AgCl(s) + NaNO3(aq)
The positive or negative ions of two ionic compounds replace each other.

(Example: Precipitation Reactions)

2 C8H18(l) + 25 O2(g) ⟶ 16 CO2(g) + 18 H2O(g)
A compound reacts with an oxidant (usually oxygen) in a highly exothermic

reaction. For hydrocarbons, the products are carbon dioxide and water.

HCl(aq) + NaOH(aq) ⟶ NaCl(aq) + H2O(l)
A proton is transferred from a proton donor (acid) to a proton acceptor (base).