1. Types of Reactions

2.  Driving Forces: 1. Formation of a solid
 2. Formation of water
 3. Transfer of electrons
 4. Formation of a gas
 When two or more reactants are brought
together, and one or more of the above
outcomes can occur, a reaction is likely

3.  Reactions driven by tendency of metals to
donate electrons to nonmetals; these
reactions involve the formation of ions
discussed in Chapter 4
◦ e.g., 2Na (s) + Cl2 (g)  NaCl (s) [ Na+ + Cl- ]
◦ 2Mg (s) + O2 (g)  2MgO (s) [Mg2+ + O2-]
◦ 2Al (s) + Fe2O3 (s)  2Fe (s) + Al2O3 (s)
 Al  Al3+ + 3e-
 Fe3+ + 3e-  Fe

6. ◦ 2Na (s) + Cl2 (g)  2 NaCl (s)
 Na0 Cl0 Na+1 Cl-1
◦ 2Mg (s) + O2 (g)  2MgO (s)
 Mg0 O0 Mg+2 O-2
◦ 2Al (s) + Fe2O3 (s)  2Fe (s) + Al2O3 (s)
 Al0 Fe+3 O-2 Fe0 Al+3 O-2


7.  Combustion: oxidation-reduction reactions involving
oxygen that produce heat so quickly that a flame is also
produced
 e.g. CH4 (g) + 2O2(g)  CO2 (g) + 2H2O (g)
  usually used to produce heat or electricity

 Synthesis/Combination Reactions: synthesis of a new
compound; also a subclass of oxidation-reduction reactions
 N2 (g) + O2 (g)  2NO (g)
 Mg (s) + F2 (g)  MgF2 (s)

 Decomposition Reactions: compound broken down into
simpler compounds or elements; also a subclass of oxidation-
reduction reactions
 usually accomplished by heating or electrical current
 2H2O (l)  H2 (g) + O2 (g)

8. Combustion of Methane
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