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March 16, 2010

March 16, 2010. Complete the Warm up at your table (Synthesis Table) Once you are done with the warm up, get a packet from the front of the room Start the packet in class and finish it for H/W Today we will be discussing: “How do you recognize and represent chemical changes?”. Homework:

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March 16, 2010

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  1. March 16, 2010 • Complete the Warm up at your table (Synthesis Table) • Once you are done with the warm up, get a packet from the front of the room • Start the packet in class and finish it for H/W • Today we will be discussing: “How do you recognize and represent chemical changes?” Homework: Synthesis W/S Important Dates: 4/2: Reaction Test

  2. March 16, 2010 • We will be taking the quiz first! • Complete the Warm up at your table (Balancing Reactions) • You will need paper and something to write with • Today we will be discussing: “How do you recognize and represent chemical changes?” Important Dates: 4/2: Reaction Test Homework: Single and Combustion. W/S

  3. Combustion • Combustion Reactions: • Reactions in which oxygen combines with a hydrocarbon molecule and releases energy in the form of heat and light • C3H6O(s) + 3O2(g) → 3CO2(g) + 3H2O(g) • CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)

  4. Predicting Combustion Products • Products will ALWAYS be Carbon Dioxide and Water • All reactants and Products will be gasses • C3H8(g) + O2(g) → CO2(g) + H2O(g) • Balancing Trick! • 1. Balance the carbons using carbons subscript • 2. Balance the hydrogens using hydrogens subscript/2 • 3. Add up all the oxygens on the product side. Balance the oxygens using this number/2

  5. Predicting Combustion Products • C3H8(g) + O2(g) → CO2(g) + H2O(g) • C3H8(g) + 10/2O2(g) → 3CO2(g) + 4H2O(g) • C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) • Balancing Trick! • 1. Balance the carbons using carbons subscript • 2. Balance the hydrogens using hydrogens subscript/2 • 3. Add up all the oxygens on the product side. Balance the oxygens using this number/2

  6. Combustion Practice • C8H16(g) + O2(g) → CO2(g) + H2O(g) • C8H16(g) + 12O2(g) → 8CO2(g) + 8H2O(g) • C21H44(g) + O2(g) → CO2(g) + H2O(g) • C21H44(g) + 32O2(g) → 21CO2(g) + 22H2O(g) • C6H14(g) + O2(g) → CO2(g) + H2O(g) • C6H14(g) + 19/2O2(g) → 6CO2(g) + 7H2O(g) • C6H14(g) + 19O2(g) → 12CO2(g) + 14H2O(g) • C3H6O(g) + O2(g) → CO2(g) + H2O(g) • C3H6O(g) + 4O2(g) → 3CO2(g) + 3H2O(g)

  7. Single Replacement • Single Replacement Reactions: • A reaction in which the atoms of one element replace the atoms of another element in a compound • AB + C → CB + A • Cu(S) + 2AgNO3(aq) → 2Ag(s) + Cu(NO3)2(aq) • F2(g) + 2NaBr(aq) → 2NaF(aq) + Br2(l)

  8. Activation Series • Lithium • Rubidium • Potassium • Calcium • Sodium • Magnesium • Aluminum • Manganese • Zinc • Iron • Nickel • Tin • Lead • Copper • Silver • Platinum • Gold • Fluorine • Chlorine • Bromine • Iodine • Page 293

  9. Single Replacement Products • 3 basic types of single replacement reactions • 1. Metal replaced by a more active metals • 2. Hydrogen in acids replaced by active metals • 3. Nonmetals replaced by more active nonmetals • 4. Hydrogen in water replaced by a metal

  10. Metalreplaced by a more active Metals • MNM + AM → AMNM + M • Fe(s) +  CuSO4(aq)  →    FeSO4(aq)  +  Cu(s) • Na(s) + SnCO3 → ? • 2Na(s) + SnCO3 → Na2CO3 + Sn(s) • Pt(s) + Zn2O → ? • Pt(s) + Zn2O → NR

  11. Hydrogeninacidsreplaced by active metals • M(s) + HX → MX + H2(g) • Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) • Cu(s) + HNO3(aq) → Cu(NO3)2(aq) + H2(g) • Cu(s) + 2HNO3(aq) → Cu(NO3)2(aq) + H2(g) • Na(s) + H2SO4(aq) → Na2SO4(aq) + H2(g) • 2Na(s) + H2SO4(aq) → Na2SO4(aq) + H2(g)

  12. Nonmetalsreplaced by more active nonmetals • NM(s,l,g) + MNM(aq) → MNM(aq) + NM(s,l,g) • Cl2(g) + 2NaBr(aq) → 2NaCl(aq) + Br2(l) • Br2(l) + MgI2(aq) → ? • Br2(l) + MgI2(aq) → MgBr2(aq) + I2(s) • F2(g) + FeBr2(aq) → ? • F2(g) + FeBr2(aq) → NR

  13. HydrogeninWaterreplaced by a Metal • M(s) + H2O(l) → M(OH)x(aq) + H2(g) • 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g) • Fe(s) + H2O(l) → ? • Fe(s) + 2H2O(l) → Fe(OH)2(aq) + H2(g) • Sr(s) + H2O(l) → ? • Sr(s) + 2H2O(l) → Sr(OH)2(aq) + H2(g)

  14. Single Replacement Practice • Al(s) + H2SO4(aq) → ? • 2Al(s) + 3H2SO4(aq) → 3H2(g) + Al2(SO4)3(aq) • Br2(l) + MgI2(aq) → ? • Br2(l) + MgI2(aq) → MgBr2(aq) + I2(s) • Zn(s) + H2O(l) → ? • Zn(s) + 2H2O(l) → ZnOH(aq) +H2(g) • Ag(s) + CuCl2(aq) → ? • Ag(s) + CuCl2(aq) → NR • Fe(s) + CuSO4 → ? • Fe(s) + CuSO4 → FeSO4 + Cu(s) • Br2(g) + KCl(aq) → ? • Br2(g) + KCl(aq) → NR

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