1. Types of Chemical Reactions Single Replacement Reactions Double Replacement Reactions Combustion Reactions

2. Recall Synthesis Reactions Two or more substances combine to form one substance. Two or more substances combine to form one substance. The general form is ______________ The general form is ______________ Decomposition Reactions One substance reacts to form two or more substances. One substance reacts to form two or more substances. The general form is ______________ The general form is ______________

3. Single Replacement Reactions A metal will replace a metal ion in a compound. A metal will replace a metal ion in a compound. The general form is ______________ The general form is ______________ A nonmetal will replace a nonmetal ion in a compound. A nonmetal will replace a nonmetal ion in a compound. The general form is ______________ The general form is ______________

4. Single Replacement Reactions Examples: Examples: Ni + AgNO 3  Ni + AgNO 3  Nickel replaces the metallic ion Ag + (metal replaces metal ion) Nickel replaces the metallic ion Ag + (metal replaces metal ion) The silver becomes free silver and the nickel becomes the nickel (II) ion. The silver becomes free silver and the nickel becomes the nickel (II) ion. Ni + AgNO 3  Ag + Ni(NO 3 ) 2 Ni + AgNO 3  Ag + Ni(NO 3 ) 2 Balance the equation: Balance the equation: Ni + 2AgNO 3  2Ag + Ni(NO 3 ) 2 Ni + 2AgNO 3  2Ag + Ni(NO 3 ) 2

5. Thermite Reaction Steve Spangler Video Thermite Steve Spangler Video Thermite

6. Thermite Reaction Al + Fe 2 O 3  Al + Fe 2 O 3  Aluminum will replace iron (III) as was seen in the video. Aluminum will replace iron (III) as was seen in the video. Iron (III) becomes Fe and aluminum metal becomes Al 3+. Iron (III) becomes Fe and aluminum metal becomes Al 3+. 2Al + Fe 2 O 3  ______________ 2Al + Fe 2 O 3  ______________

7. Double Replacement Reactions Ions of two compounds exchange places with each other. Ions of two compounds exchange places with each other. Reactants must be two ______________, in aqueous solution Reactants must be two ______________, in aqueous solution The general form is ______________ The general form is ______________

8. Remember the Demonstration!!!!!!!! Word - Lead (II) Nitrate + Potassium Iodide --> Potassium Nitrate + Lead Iodide Skeletal - Pb(NO 3 ) 2 (aq) + 2KI (aq) --> 2KNO 3 (aq) + PbI 2 (s) What occurred??? This is a double displacement reaction

9. Double Replacement NaOH + CuSO 4  NaOH + CuSO 4  The Na + and Cu 2+ switch places. The Na + and Cu 2+ switch places. Na + combines with SO 4 2- to form Na 2 SO 4. Na + combines with SO 4 2- to form Na 2 SO 4. Cu 2+ combines with OH - to form Cu(OH) 2 Cu 2+ combines with OH - to form Cu(OH) 2 NaOH + CuSO 4  ______________ NaOH + CuSO 4  ______________ 2NaOH + CuSO 4  ______________ 2NaOH + CuSO 4  ______________

10. Double Replacement CuSO 4 + Na 2 CO 3  CuSO 4 + Na 2 CO 3  Cu 2+ combines with CO 3 2- to form ______________. Cu 2+ combines with CO 3 2- to form ______________. Na + combines with SO 4 2- to form ______________. Na + combines with SO 4 2- to form ______________. CuSO 4 + Na 2 CO 3  ______________ CuSO 4 + Na 2 CO 3  ______________

11. Double Replacement Reactions Think about it like “foil”ing in algebra, first and last ions go together + inside ions go together Example: AgNO 3(aq) + NaCl (s)  AgCl (s) + NaNO 3(aq) Another example: K 2 SO 4(aq) + Ba(NO 3 ) 2(aq)  KNO 3(aq) + BaSO 4(s) 2

12. Recognition You need to be able to recognize which reaction is taking place You need to be able to recognize which reaction is taking place

13. Practice Examples: H 2 + O 2  H 2 + O 2  H 2 O  H 2 O  Zn + H 2 SO 4  Zn + H 2 SO 4  HgO  HgO  KBr + Cl 2  KBr + Cl 2  AgNO 3 + NaCl  AgNO 3 + NaCl  Mg(OH) 2 + H 2 SO 3  Mg(OH) 2 + H 2 SO 3  _____________

14. Combustion Reactions Combustion means “ _________ ” Normally, a compound composed of only C, H, (and maybe O) is reacted with oxygen – usually called “ _________ ” Combustion means “ _________ ” Normally, a compound composed of only C, H, (and maybe O) is reacted with oxygen – usually called “ _________ ” If the combustion is _________, the products will be CO 2 and H 2 O. If the combustion is _________, the products will be CO 2 and H 2 O. If the combustion is _________,, the products will be CO (or possibly just C) and H 2 O. If the combustion is _________,, the products will be CO (or possibly just C) and H 2 O.

15. Combustion Reaction When a substance combines with oxygen, a combustion reaction results. When a substance combines with oxygen, a combustion reaction results. The combustion reaction may also be an example of an earlier type such as 2Mg + O 2  2MgO. The combustion reaction may also be an example of an earlier type such as 2Mg + O 2  2MgO. The combustion reaction may be burning of a fuel. The combustion reaction may be burning of a fuel.

16. Combustion Reactions Combustion reactions involve light and heat energy released. Combustion reactions involve light and heat energy released. Natural gas, propane, gasoline, etc. are burned to produce heat energy. Natural gas, propane, gasoline, etc. are burned to produce heat energy. Most of these organic reactions produce _________. Most of these organic reactions produce _________.

17. Combustion Reaction When hydrocarbon compounds C x H x are burned in oxygen, the products are water and carbon dioxide. When hydrocarbon compounds C x H x are burned in oxygen, the products are water and carbon dioxide. CH 4 + O 2  CO 2 + H 2 O CH 4 + O 2  CO 2 + H 2 O CH 4 + 2O 2  CO 2 + 2H 2 O CH 4 + 2O 2  CO 2 + 2H 2 ODemonstration

18. Combustion Reactions Generally combustion reactions involve the burning of a Hydrocarbon (C x H x ) in Oxygen. Generally combustion reactions involve the burning of a Hydrocarbon (C x H x ) in Oxygen. Other elements can also burn with Oxygen Other elements can also burn with Oxygen 2Mg + O 2  _________ + Energy 2Mg + O 2  _________ + Energy 2H 2 + O 2  _________ + Energy (basis behind fuel cell energy) 2H 2 + O 2  _________ + Energy (basis behind fuel cell energy) P 4 + 5O 2  P 4 O 10 + Energy (matches) P 4 + 5O 2  P 4 O 10 + Energy (matches)

19. Practice Classify each of the following as to type: Classify each of the following as to type: H 2 + Cl 2  2HCl H 2 + Cl 2  2HCl _________ _________ Ca + 2H 2 O  Ca(OH) 2 + H 2 Ca + 2H 2 O  Ca(OH) 2 + H 2 _________ _________

20. Practice 2CO + O 2  2CO 2 2CO + O 2  2CO 2 _________ _________ 2KClO 3  2KCl + 3O 2 2KClO 3  2KCl + 3O 2 _________ _________

21. Practice FeS + 2HCl  FeCl 2 + H 2 S FeS + 2HCl  FeCl 2 + H 2 S _________ _________ Zn + HCl  ? ______ + ______ Zn + HCl  ? ______ + ______ __________ __________