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Types of chemical Reactions

Types of chemical Reactions. Type one. 2H 2(g) + O 2(g) ----> 2H 2 O (g) C (s) + O 2(g) ----> CO 2(g) CaO (s) + H 2 O (l) ----> Ca(OH) 2(s). Combination: When two or more simple compounds combine to form a more complicated one A + B ---> AB Ex: 8 Fe + S 8 ---> 8 FeS. Type two.

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Types of chemical Reactions

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  1. Types of chemicalReactions

  2. Typeone • 2H2(g) + O2(g) ----> 2H2O(g) • C(s) + O2(g) ----> CO2(g) • CaO(s) + H2O(l) ----> Ca(OH)2(s) • Combination: • When two or more simple compounds combine to form a more complicated one • A + B ---> AB • Ex: • 8 Fe + S8 ---> 8 FeS

  3. Typetwo • Cu + 2AgNO3 → 2Ag + Cu(NO3)2 • Fe + Cu(NO3)2 → Fe(NO3)2 + Cu • Ca + 2H2O → Ca(OH)2 + H2 • Zn + 2HCl → ZnCl2 + H2 • Single Displacement: • When one element trades places with another element in a compound • A + BC ---> AC + B • Ex: • Mg + 2 H2O ---> Mg(OH)2 + H2

  4. Typethree • KOH + H2SO4 ---> K2SO4 + H2O • FeS + HCl ---> FeCl2 + H2S • NaCl + H2SO4 ---> Na2SO4 + HCl • AgNO3 + NaCl ---> AgCl + NaNO3 • Double Displacement: • When the anions and cations of two different molecules switch places, forming two entirely different compounds • AB + CD ---> AD + CB • Ex: • Pb(NO3)2 + 2 KI ---> PbI2 + 2 KNO3

  5. Typefour • C12H22O11(s) ----> 12C(s) + 11H2O(g) • Pb(OH)2(cr) ----> PbO(cr) + H2O(g) • 2Ag2O(cr) ----> 4Ag(cr) + O2(g) • Decompostion: • When complex molecule breaks down to make simpler ones • AB ---> A + B • Ex: • 2 H2O ---> 2 H2 + O2

  6. Typefive • CH4(g) + 2O2(g) ----> 2H2O(g) + CO2(g) • 2C2H6(g) + 7O2(g) ----> 6H20(g) + 4CO2(g) • C3H8(g) + 5O2(g) ----> 4H2O(g) + 3CO2(g) • Combustion: • When oxygen combines with another compound to form water and carbon dioxide • ABC (hydrocarbon)+ XO2 • --->YH2O+ ZCO2 • Ex: • C10H8 + 12 O2 ---> 10 CO2 + 4 H2O

  7. Special Case #1 Acid Base • HCl + NaOH ---> NaCl + H2O • H2SO4 + 2KOH ---> K2SO4 + 2H2O • 2HNO3 + Ca(OH)2 ---> Ca(NO3)2 + 2H2O • CH3COOH + NaOH ---> NaOOCCH3 + H2O Acid/Base: When an acid and base react with each other. The H+ ion in the acid reacts with the OH- ion in the base, causing the formation of water HA + BOH ---> H2O + BA Ex: HBr + NaOH ---> NaBr + H2O

  8. Special Case #2 Redox • 1 Fe + 3 NaBr --> FeBr3 + 3 Na • Fe0 + 3(Na+ Br- -) --> Fe 3+ (Br -)3 + 3 Na 0 • Iron oxidizes charge goes up • Sodium reduces charge goes down • When reactants and products charge changes.

  9. Yes to a question means stop • 4)  New compound forms and a new element remains? • Single replacement reaction • 5)  If you haven't answered "yes" to any of the questions above. • Double displacement reaction • Special Cases: • #1 Acid Base a form of double displacement Water is Product and Reactants have • HA + B(OH) > H2O + BA • #2 Redox – All Combination, single replacement, and some double displacements, and decompositions • (Does an valence change value) • 1)  Does your reaction have oxygen as one of it's reactants and carbon dioxide and water as products? • Combustion reaction • 2)  Does your reaction have two (or more) chemicals combining to form one chemical? • Combination reaction • 3)  Does your reaction have one large molecule falling apart to make several small ones? • Decomposition reaction

  10. Practice :List what type the following reactions are • 1)  NaOH + KNO3 --> NaNO3 + KOH • 2)  CH4 + 2 O2 --> CO2 + 2 H2O • 3)  1 Fe + 3 NaBr --> FeBr3 + 3 Na • 4)  CaSO4 + Mg(OH)2 --> Ca(OH)2 + MgSO4 • 5)  NH4OH + HBr --> H2O + NH4Br • 6)  Pb + O2 --> PbO2 • 7)  Na2CO3 --> Na2O + CO2

  11. Answerstopractice • 1)  NaOH + KNO3 --> NaNO3 + KOH • 2)  CH4 + 2 O2 --> CO2 + 2 H2O • 3)  2 Fe + 6 NaBr --> 2 FeBr3 + 6 Na • 4)  CaSO4 + Mg(OH)2 --> Ca(OH)2 + MgSO4 • 5)  NH4OH + HBr --> H2O + NH4Br • 6)  Pb + O2 --> PbO2 • 7)  Na2CO3 --> Na2O + CO2 • 1)  double displacement 2)  combustion – redox Carbon Oxidized;Oxygen reduced3)  single replacement - redox iron Oxidized; Sodium reduced 4)  double displacement 5)  acid-base 6)  Combining - redox lead Oxidized; Oxygen reduced 7)  decomposition

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