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Chemical Reactions

Chemical Reactions. http://ssis-chem.wikispaces.com/file/view/mgburnpic.jpg. http://www.reviseguys.com/moodle/course/view.php?id=10. Chemical Reaction. Chemical change = chemical reaction Changes may be visible: color change cloudiness (precipitation) gas formed (bubbles and/or odor)

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Chemical Reactions

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  1. Chemical Reactions http://ssis-chem.wikispaces.com/file/view/mgburnpic.jpg http://www.reviseguys.com/moodle/course/view.php?id=10 CHM 1010 PGCC Barbara Gage

  2. Chemical Reaction • Chemical change = chemical reaction Changes may be visible: • color change • cloudiness (precipitation) • gas formed (bubbles and/or odor) • reactant decreases (without dissolving) • energy is released or absorbed CHM 1010 PGCC Barbara Gage

  3. Chemical Equations • Chemical changes can be written symbolically. The symbolic representation is called a chemical equation. Carbon reacts with oxygen to form carbon dioxide. C + O2 CO2 reactants products CHM 1010 PGCC Barbara Gage

  4. Chemical Equations • Reaction arrows can go in either direction: 2 H2 + O2 2 H2O • Or both directions: NH4OH  NH3 + H2O CHM 1010 PGCC Barbara Gage

  5. Or… CHM 1010 PGCC Barbara Gage

  6. Chemical Equations • Because of the Law of Conservation of Matter, you must account for all atoms in a chemical change. Carbon reacts with oxygen to form carbon monoxide. C + O2 CO 2C + O2 2 CO coefficient Equation is now balanced. CHM 1010 PGCC Barbara Gage

  7. Chemical Equations • A sample of propane, C3H8, when ignited with oxygen produces carbon dioxide and water. C3H8 + O2 CO2 + H2O C3H8 + 5 O2 3 CO2 + 4 H2O CHM 1010 PGCC Barbara Gage

  8. Chemical Reactions Al + O2 Al2O3 CaCO3 + HI  CaI2 + CO2 + H2O Na3PO4 + BaCl2  NaCl + Ba3(PO4)2 C4H10 + O2  CO2 + H2O CHM 1010 PGCC Barbara Gage

  9. Chemical Equations • If you have information on the states of matter, that can be added to the equation. s = solid l = liquid g = gas aq = aqueous Aqueous silver nitrate reacts with aqueous potassium chloride to form solid silver chloride and aqueous potassium nitrate. AgNO3(aq) + KCl(aq)  AgCl(s) + KNO3(aq) CHM 1010 PGCC Barbara Gage

  10. Balancing Tips… • Balance polyatomic ions that stay intact as a single unit. • Leave hydrogens and oxygens to the last (oxygen very last) • Be sure to reduce the coefficients to the smallest whole numbers. CHM 1010 PGCC Barbara Gage

  11. Before • Write the balanced chemical equation for the change in the boxes and indicate the reaction type. After CHM 1010 PGCC Barbara Gage

  12. Let’s look at the lab rxns… • Mg (s) + HCl(aq) -------> • CuCO3 (s) ----------> • Mg (s) + -------------> • NaHCO3 (s) + HCl (aq)-----> • CuSO4 (aq) + Fe (s) --------> CHM 1010 PGCC Barbara Gage

  13. Let’s look at the lab rxns… • CoCl2 (aq) + Na3PO4 (aq) –> • KClO3 (s) + ---------> • Fe (s) + ----------> • HCl (aq) + NaOH (aq) ----> CHM 1010 PGCC Barbara Gage

  14. Mg (s) + 2 HCl (aq) -------> MgCl2 (aq) + H2 (g) • CuCO3 (s) + -------------> CuO (s) + CO2 (g) • 2Mg (s) + O2 (g) -------------> 2MgO (s) • NaHCO3 (s) + HCl (aq)---> NaCl (aq) + H2CO3 (aq) ----> NaCl(aq) + H2O (l) + CO2 (g) • CuSO4 (aq) + Fe (s) --------> Cu (s) + FeSO4 (aq) • 3CoCl2(aq) + 2Na3PO4(aq) –>Co3(PO4)2(s) + 6NaCl (aq) • 2KClO3 (s) + -----------------> 2 KCl (s) + 3 O2 (g) • 2Fe (s) + O2 (g) ---------------> 2 FeO (s) • HCl (aq) + NaOH (aq) ----> NaCl (aq) + H2O (l) CHM 1010 PGCC Barbara Gage

  15. Types of Reactions • 1) Combination or Synthesis • elements or (element + compound) or compounds ------> compound • Fe (s) + S (s) ------> FeS (s) • O2 (g) + 2 CO (g) ------> 2 CO2 (g) • H2O (l) + SO3 (g) ------> H2SO4 (aq) CHM 1010 PGCC Barbara Gage

  16. Mg (s) + 2 HCl (aq) -------> MgCl2 (aq) + H2 (g) • CuCO3 (s) + -------------> CuO (s) + CO2 (g) • 2Mg (s) + O2 (g) -------------> 2MgO (s) • NaHCO3 (s) + HCl (aq)---> NaCl (aq) + H2CO3 (aq) ----> NaCl(aq) + H2O (l) + CO2 (g) • CuSO4 (aq) + Fe (s) --------> Cu (s) + FeSO4 (aq) • 3CoCl2(aq) + 2Na3PO4(aq) –>Co3(PO4)2(s) + 6NaCl (aq) • 2KClO3 (s) + -----------------> 2 KCl (s) + 3 O2 (g) • 2Fe (s) + O2 (g) ---------------> 2 FeO (s) • HCl (aq) + NaOH (aq) ----> NaCl (aq) + H2O (l) CHM 1010 PGCC Barbara Gage

  17. Types of Reactions • 2) Decomposition or Analysis • compound ------> elements or (element and compound) or compounds • 2 HgO (s) -----> 2Hg (l) + O2 (g) • 2 KBrO3 (s) -----> 2 KBr (s) + 3 O2 (g) • CaCO3 (s) ------> CaO (s) + CO2 (g) CHM 1010 PGCC Barbara Gage

  18. Mg (s) + 2 HCl (aq) -------> MgCl2 (aq) + H2 (g) • CuCO3 (s) + -------------> CuO (s) + CO2 (g) • 2Mg (s) + O2 (g) -------------> 2MgO (s) • NaHCO3 (s) + HCl (aq)---> NaCl (aq) + H2CO3 (aq) ----> NaCl(aq) + H2O (l) + CO2 (g) • CuSO4 (aq) + Fe (s) --------> Cu (s) + FeSO4 (aq) • 3CoCl2(aq) + 2Na3PO4(aq) –>Co3(PO4)2(s) + 6NaCl (aq) • 2KClO3 (s) + -----------------> 2 KCl (s) + 3 O2 (g) • 2Fe (s) + O2 (g) ---------------> 2 FeO (s) • HCl (aq) + NaOH (aq) ----> NaCl (aq) + H2O (l) CHM 1010 PGCC Barbara Gage

  19. Types of Reactions • 3) Single Replacement • element + compound --------> element + compound • Cu (s) + 2AgNO3 (aq) ---->2Ag (s) + Cu(NO3)2 (aq) CHM 1010 PGCC Barbara Gage

  20. Mg (s) + 2 HCl (aq) -------> MgCl2 (aq) + H2 (g) • CuCO3 (s) + -------------> CuO (s) + CO2 (g) • 2Mg (s) + O2 (g) -------------> 2MgO (s) • NaHCO3 (s) + HCl (aq)---> NaCl (aq) + H2CO3 (aq) ----> • NaCl (aq) + H2O (l) + CO2 (g) • CuSO4 (aq) + Fe (s) --------> Cu (s) + FeSO4 (aq) • 3CoCl2(aq) + 2Na3PO4(aq) –>Co3(PO4)2(s) + 6NaCl (aq) • 2KClO3 (s) + -----------------> 2 KCl (s) + 3 O2 (g) • 2Fe (s) + O2 (g) ---------------> 2 FeO (s) • HCl (aq) + NaOH (aq) ----> NaCl (aq) + H2O (l) CHM 1010 PGCC Barbara Gage

  21. Types of Reactions • 4)Double Replacement compound + compound —> compound +compound AgNO3 (aq) + NaCl (aq) —> AgCl (s) +NaNO3 (aq) • Double Replacement Rxns: Solid forming AgNO3 (aq) + NaCl (aq) —> AgCl (s) +NaNO3 (aq) Gas-forming KHCO3 (aq) + HCl (aq) ----> KCl (aq) + CO2 (g) +H2O (l) Acid-Base HCl (aq) + KOH (aq) ----> KCl (aq) + H2O (l) CHM 1010 PGCC Barbara Gage

  22. Mg (s) + 2 HCl (aq) -------> MgCl2 (aq) + H2 (g) • CuCO3 (s) + -------------> CuO (s) + CO2 (g) • 2Mg (s) + O2 (g) -------------> 2MgO (s) • NaHCO3 (s) + HCl (aq)---> NaCl (aq) + H2CO3 (aq) ----> • NaCl (aq) + H2O (l) + CO2 (g) • CuSO4 (aq) + Fe (s) --------> Cu (s) + FeSO4 (aq) • 3CoCl2(aq) + 2Na3PO4(aq) –>Co3(PO4)2(s) + 6NaCl (aq) • 2KClO3 (s) + -----------------> 2 KCl (s) + 3 O2 (g) • 2Fe (s) + O2 (g) ---------------> 2 FeO (s) • HCl (aq) + NaOH (aq) ----> NaCl (aq) + H2O (l) CHM 1010 PGCC Barbara Gage

  23. Types of Reactions • 5) Oxidation-Reduction (redox) CH4 (g) + 2O2 (g) ----> CO2 (g) + 2H2O (l) 2Mg (s) + O2 (g) -----------> 2MgO (s) 4HCl (aq) + 3FeCl2 (aq) + KMnO4(aq) --> MnO2(s) + KCl(aq) + 3FeCl3(aq) + 2H2O(l) CHM 1010 PGCC Barbara Gage

  24. Mg (s) + 2 HCl (aq) -------> MgCl2 (aq) + H2 (g) CuCO3 (s) + -------------> CuO (s) + CO2 (g) 2Mg (s) + O2 (g) -------------> 2MgO (s) NaHCO3 (s) + HCl (aq)---> NaCl (aq) + H2CO3 (aq) ----> NaCl (aq) + H2O (l) + CO2 (g) CuSO4 (aq) + Fe (s) --------> Cu (s) + FeSO4 (aq) 3CoCl2(aq) + 2Na3PO4(aq) –>Co3(PO4)2(s) + 6NaCl (aq) 2KClO3 (s) + -----------------> 2 KCl (s) + 3 O2 (g) 2Fe (s) + O2 (g) ---------------> 2 FeO (s) HCl (aq) + NaOH (aq) ----> NaCl (aq) + H2O (l) CHM 1010 PGCC Barbara Gage

  25. Solubility Rules • Reactants and products of reactions may be soluble. • Use solubility rules to label them. CHM 1010 PGCC Barbara Gage

  26. Solubility Rules Soluble Ionic Compounds • All common compounds of Group IA (1) ions and ammonium ion are soluble. • All common nitrates, acetates, and most perchlorates are soluble. • All common chlorides, bromides, and iodides are soluble, except for those of silver (I), lead (II), copper (I) and mercury (I). All common fluorides are soluble except those of lead (II) and Group IIA (2). • All common sulfates are soluble except those of calcium, strontium, barium, silver (I), and lead (II). Insoluble Ionic Compounds • All common metal hydroxides are insoluble, except those of Group IA (1) and the larger members of Group IIA (2) (beginning with calcium). • All carbonates and phosphates are insoluble, except those of Group IA (1) and ammonium ion. • Most other combinations not mentioned above (such as chromates, oxides, sulfides) are insoluble, except those of Group IA (1) and ammonium ion. CHM 1010 PGCC Barbara Gage

  27. Predicting Reactions… • Complete and balance the following: copper(II) chloride reacts with sodium hydroxide • CuCl2 (aq) + NaOH (aq)  • Double displacement reaction… CuCl2 (aq) + NaOH (aq)  Cu(OH)2 + NaCl • CuCl2 (aq) + 2 NaOH (aq)  Cu(OH)2 (s) + 2 NaCl (aq) CHM 1010 PGCC Barbara Gage

  28. Ionic reactions • Ionic compounds in solution dissociate into ions. • CuCl2 (aq) + 2 NaOH (aq)  Cu(OH)2 (s) + 2 NaCl (aq) Is actually… • Cu2+ (aq) + 2 Cl- (aq) + 2 Na+ (aq) + 2 OH-(aq) Cu(OH)2 (s) + 2 Na+ (aq) + 2 Cl- (aq) CHM 1010 PGCC Barbara Gage

  29. Net Ionic Reactions • Cu2+ (aq) + 2 Cl- (aq) + 2 Na+ (aq) + 2 OH- (aq)  Cu(OH)2 (s) + 2 Na+ (aq) + 2 Cl- (aq) • Cu2+ (aq) + 2 Cl- (aq) + 2 Na+ (aq) + 2 OH- (aq)  Cu(OH)2 (s) + 2 Na+ (aq) + 2 Cl- (aq) • Cu2+ (aq) + 2 OH- (aq)  Cu(OH)2 (s) net ionic equation CHM 1010 PGCC Barbara Gage

  30. Net Ionic Reactions • Lead (II) nitrate reacts with potassium iodide • Pb(NO3)2 + KI  • Pb(NO3)2 + KI  PbI2 + KNO3 • Pb(NO3)2 (aq) + 2 KI (aq) PbI2 (s) + 2 KNO3 (aq) • Pb2+ (aq) + 2 NO3- (aq) + 2 K+ (aq) + 2 I- PbI2 (s) + 2 K+ (aq) + 2 NO3- (aq) • Pb2+ (aq) + 2 NO3- (aq) + 2 K+ (aq) + 2 I- PbI2 (s) + 2 K+ (aq) + 2 NO3- (aq) • Pb2+ (aq) + 2 I-(aq)  PbI2 (s) net ionic equation CHM 1010 PGCC Barbara Gage

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