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TYPES OF REACTIONS

TYPES OF REACTIONS. 5 major types. SYNTHESIS DECOMPOSITION SINGLE DISPLACEMENT DOUBLE DISPLACEMENT COMBUSTION. SYNTHESIS. SYNTHESIS. A + B AB 6 types of Synth esis Reactions. SYNTHESIS: Type 1. Production of OXIDES 2Mg (s) + O 2(g) 2MgO (s) Element + oxygen OXIDE.

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TYPES OF REACTIONS

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  1. TYPES OF REACTIONS

  2. 5 major types • SYNTHESIS • DECOMPOSITION • SINGLE DISPLACEMENT • DOUBLE DISPLACEMENT • COMBUSTION

  3. SYNTHESIS

  4. SYNTHESIS • A + B AB • 6 types of Synthesis Reactions

  5. SYNTHESIS: Type 1 • Production of OXIDES • 2Mg(s) + O2(g)2MgO(s) Element + oxygen OXIDE

  6. SYNTHESIS: Type 2 • Production of BINARY COMPOUNDS • 2Na(s) + Cl2(g)2NaCl(s) Metal + non-metalBinary Comp

  7. SYNTHESIS: Type 3 • Production of an ACID • SO3(g) + H2O(l)H2SO4(aq) Non-metal oxide + WaterACID • ** Recall: Acid contains H (gets it from water)

  8. SYNTHESIS: Type 4 • Production of BASES • CaO(s) + H2O(l)Ca(OH)2 Metal oxide + waterBASE

  9. SYNTHESIS: Type 5 • Production of Metal- carbonate • CaO(s) + CO2(g)CaCO3(s) Metal oxide + CO2(g)Metal Carbonate

  10. SYNTHESIS: Type 6 • Production of variousCOMBINATIONS • 2C(s) + O2(g) 2CO(g) • C(s) + O2(g)CO2(g)

  11. DECOMPOSITION

  12. DECOMPOSITION • Opposite of Synthesis • 1 reactant 2 or more products • AB A + B • 2 types of Decomposition

  13. DECOMPOSITIONType 1 • Thermal Decomposition • Requires heat • 2H2O(l) 2H2(g) + O2(g) • ** Indicated as Δ above arrow Δ

  14. DECOMPOSITIONType 2 • Compound Other Compounds • Na2CO3Na2O + CO2 • Sodium carbonate  Sodium oxide + Carbon dioxide • Note: CARBONATES will always make a metal oxide + carbon dioxide gas

  15. CLASSWORK • Read Section 3.2 and answer • Pg 125 : 7-10, 12 • Pg 127: 21-30 • Pg 132: 13, 15, 16 • Pg 134: 31-40

  16. COMBUSTION • Reaction of a fuel with oxygen • Most of the time that fuel is a carbon-containing compound. • COMPLETE COMBUSTION produces CO2(g) and H2O(l) • INCOMPLETE COMBUSTION produces CO(g), C, CO2(g) and H2O(l) and other oxides (Eg. SO2(g) , NO2(g) )

  17. SINGLE DISPLACEMENT

  18. SINGLE DISPLACEMENT • AB + C CB + A • One metal “displaces another” • 2 types of reactions

  19. SINGLE DISPLACEMENTType 1 • Displaces METALS • Ag(NO3)(aq) + Cu(s) Cu(NO3)(aq) + Ag(s) Copper bumped silver out! • Cu(NO3)2 + Ag(s) NO REACTION • This means that Cu is MORE reactive than Ag

  20. SINGLE DISPLACEMENT • Reactivity… How do you know? • ACTIVITY SERIES tells you which metal is MORE reactive • Reaction only occurs if solo metal is MORE reactive than combined metal

  21. Highest ACTIVITY SERIES • Potassium • Sodium • Barium • Strontium • Calcium • Magnesium • Aluminum • Zinc • Iron • Nickel • Tin • Lead • Hydrogen • Copper • Arsenic • Mercury • Silver • Platinum • Gold Lowest

  22. SINGLE DISPLACEMENTType 2 • Displaces NON-METALS • CaI2(s) + Br2(l) CaBr2(s) + I2 (g) BUT • CaBr2(s) + I2(g) NO REACTION

  23. SINGLE DISPLACEMENTType 2 • CaBr2(s) + I2(g) NO REACTION • Because Bromine is MORE reactive than Iodine, reaction will not “Go” • Recall: Non metal reactivity • F2(g)> Cl2(g)> Br2(g) > I2(g)

  24. SINGLE DISPLACEMENT • When predicting products: • Treat hydrogen as a metal • Treat acids such as HCl as ionic compounds (H+ and Cl-) • Treat water as ionic with the formula H+ and OH-

  25. CLASSWORK • READ Section 3.3 • Pg 140: 19-22 • Pg 141: 41-50 • Pg 143: 25-30 • Section 4.1 • Pg 165: 1-4 • Pg 169: 1-10

  26. DOUBLE DISPLACEMENT

  27. DOUBLE DISPLACMENT • AB + CDAD + CB • A and C are cations (+) • B and D are anions (-) • Occur in a solution; aqueous environment (aq) • BOTH reactants in a DD reaction will ALWAYS be (aq) • 3 types of DD reactions

  28. DOUBLE DISPLACEMENTTYPE 1 • Formation of a PRECIPITATE • Pb(NO3)2 (aq) +2KI (aq)PbI2 (s)+ 2KNO3(aq) • How do you know that PbI2 is a solid? • USE SOLUBILITY GUIDELINES

  29. SOLUBILITY RULES • ANIONSEXCEPTIONS • Nitrates All soluble NONE • Chlorates All soluble NONE • Acetates soluble Ag+, Hg2+ • Chlorides soluble Ag+, Hg2+, Pb2+, Cu+ • Bromides soluble Ag+, Hg2+, Pb2+, Cu+ • Iodides soluble Ag+, Hg2+, Pb2+, Cu+ • Sulfates soluble Pb2+, Ba2+, Sr2+, Ca2+ • Sulfites insoluble Na+, K+, NH4+ • Sulfides insoluble Na+, K+, NH4+, Ba2+, Sr2+ • Hydroxides insoluble Na+, K+, NH4+, Ba2+, Sr2+ • Carbonates insoluble Na+, K+, NH4+ • Phosphates insoluble Na+, K+, NH4+ • Oxides insoluble Na+, K+, Ba2+, Sr2+, Ca2+ • (These ions react with water to produce hydroxides.)

  30. Predicting Precipitates… Are the following Soluble or Insoluble? • BaCl2: • Soluble (aq) • PbCl2 : • Insoluble (s) • LiNO3: • Soluble (aq) • Li2CO3 : • Insoluble (s)

  31. SOLUBILITY GUIDELINES • If BOTH products are “Soluble” or “Aqueous” then write as NO REACTION because all ions are dissolved

  32. DOUBLE DISPLACEMENTTYPE 2 • Production of a GAS • 2 step process

  33. DOUBLE DISPLACEMENTTYPE 2 • Step 1: DD reaction • Na2CO3(aq) + 2HCl(aq) 2NaCl (aq) + H2CO3(aq) • Step 2: one product decomposes to make a gas • H2CO3(aq)H2O(l) + CO2(g)

  34. DOUBLE DISPLACEMENTTYPE 2 • OVERALL: Na2CO3(aq) + 2HCl(aq) 2NaCl (aq) + H2O(l) + CO2(g)

  35. DOUBLE DISPLACEMENTTYPE 2 • Can also result in NH3 gas • NH4Cl(aq) + NaOH(aq) NH4OH(aq) + NaCl(aq) • NH4OH(aq) NH3(g) + H2O(l) • OVERALL… NH4Cl(aq) + NaOH(aq)NaCl(aq)+ NH3(g) + H2O(l)

  36. DOUBLE DISPLACEMENTTYPE 3 • Formation of WATER in a neutralization reaction • Acid + Base Water + Salt • HNO3(aq) + NaOH(aq) NaNO3(aq) + H2O(l)

  37. HOMEWORK • Read Section 4.2 • Pg 173: 7-12 • Pg 175: 11-20 • Pg 177: 13, 16, 17, 18 • Pg 179: 21-30

  38. HOMEWORK • Page 124 # 17, 19 • Page 131 # 22, 23, 24 • Page 134 # 25 • Page 135 # 27, 28 • Page 140 # 1,2,4

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