1. Types of Chemical Reactions
Unit 5A

2. Synthesis Reaction
2 or more substances combining to form a single compound
A + B → AB
N2(g) + 3H2(g) → 2NH3(g)

3. Decomposition Reaction
A single reactant breaks down into simpler substances.
CD → C + D
2H2O2(l) → 2H2O(l) + O2(g)

4. Single- replacement Reaction
An element replaces another in an ionic compound.
E + FG → F + EG
L + JK → K + JL
2Na(s) + MgCl2(aq) → Mg(s) + 2NaCl(aq)
2F2(g) + 2FeBr3(aq) → 3Br2(l) + 2FeF2(aq)

5. Single- replacement Reactions
Only occur if the element doing the replacing is more active (reactive) than the other element!

6. Each element can replace all the other elements below it!
Activity Series of the Elements
Activity Series of the Elements
METALS NON-METALS (halogens)
Lithium Fluorine
Potassium Chlorine
Calcium Bromine
Sodium Iodine
Magnesium
Aluminum
Zinc
Chromium
Iron
Nickel
Tin
Lead
“Hydrogen”
Copper
Mercury
Silver
Platinum
Each element can replace all the other elements below it!

7. Double- replacement Reactions
The cations of 2 ionic compounds exchange anions.
QR + ST → QT + SR
BaBr2(aq) + 2AgNO3(aq) → Ba(NO3)2(aq) + 2AgBr(s)

8. Combustion Reaction
A hydrocarbon is burned with oxygen to produce carbon dioxide, water and light/ heat.
CxHy + O2(g) → CO2(g) + H2O(g)
2C4H10(l) + 13O2(g) → 8CO2(g) + 10H2O(g)
2C2H5OH(l) + 7O2(g) → 4CO2(g) + 6H2O(g)