1. Chapter 6: Classifying
Chemical Reactions

2. 1. Synthesis Reactions (Combination)
2 or more substances combine to form a compound
General Formula:
A + B  AB
1 PRODUCT
e.g.
S + O2  SO2
2SO2 + O2  2SO3
SO3 + H2O  H2SO4

3. 2. Decomposition Reactions
1 substance breaks down into 2 or more simpler substances
General Formula:
AB  A + B
1 REACTANT
e.g.
SO2  S + O2
2SO3  2SO2 + O2
H2SO4  SO3 + H2O

4. 3. Single Replacement Reactions
A combined element in a compound is replaced by an uncombined element.
General Formula:
Z + AB  AZ + B
Metals replace metals; Non-metals replace Non-metals
e.g.
Br2 + 2NaCl  2NaBr + Cl2
2Al + Fe2O3  2Fe + Al2O3
Try Practice Problems p.261 #1(ac), 2

5. 4. Double Replacement Reactions
Elements in different compounds replace each other (change places)
General Formula:
AB + XY  AY + XB
e.g.
2KI + Pb(NO3)2  PbI2 + 2KNO3
One of the products often forms a precipitate. (an insoluble solid that separates from the solution)
Try Practice Problems p.262 #1(ac), 2

6. Brad + Angelina  Bradgenlina
Bradgelina  Brad + Angelina
Brad with Jen + Angelina  Brad with Angelina + Jen

7. 5. Neutralization (Acid-Base)
A type of double replacement reaction that involves an acid reacting with a base to produce water and a salt.
General Formula:
Acid + Base  Water + Salt
e.g.
HCl + NaOH  HOH + NaCl

8. 6. Combustion https://www.youtube.com/watch?v=98Vkl1YnNFs
A special type of fast exothermic reaction where oxygen is a reactant, oxides are produced, and a large amount of energy is released.
* This reaction is the burning of methane gas (CH4)
e.g.
CH4(g) + 2O2(g)  CO2(g) + 2H2O(l) + energy
2H2(g) + O2(g)  2H2O(l) + energy
* Rockets are launched by this reaction
2Mg(s) + O2(g)  2MgO(s) + energy
* Light from flares comes from this reaction