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Unit 1 presentation Unit 1 presentation Presentation Transcript

  • Types of Reactions
  •  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
  •  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
  • ◦ 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
  •  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)
  • Combustion of MethaneThanks to www.boundless.com for the image Creative Commons Attribution- ShareAlike 3.0 Unported License